Podcast
Questions and Answers
Which factor does NOT directly affect the rate of a chemical reaction, as outlined in the provided material?
Which factor does NOT directly affect the rate of a chemical reaction, as outlined in the provided material?
- The nature of the reactants involved.
- The volume of the reaction vessel. (correct)
- The concentration of the reactants.
- The presence of a catalyst.
What is the primary role of a catalyst in a chemical reaction?
What is the primary role of a catalyst in a chemical reaction?
- To be consumed during the reaction, altering the final product.
- To increase the activation energy required for the reaction.
- To increase the reaction rate without being consumed in the process. (correct)
- To shift the equilibrium of the reaction towards the reactants.
According to the material, how does increasing the temperature typically affect the rate of a chemical reaction?
According to the material, how does increasing the temperature typically affect the rate of a chemical reaction?
- It increases the reaction rate. (correct)
- It may increase or decrease the reaction rate depending on the specific reaction.
- It has no effect on the reaction rate.
- It decreases the reaction rate.
What observation from the lab activity directly indicates the completion of the reaction between potassium permanganate and oxalic acid?
What observation from the lab activity directly indicates the completion of the reaction between potassium permanganate and oxalic acid?
Which of the following statements correctly describes the relationship between reaction rate and reactant concentration?
Which of the following statements correctly describes the relationship between reaction rate and reactant concentration?
In the experiment with chalk (CaCO3) and hydrochloric acid (HCl), what is the purpose of crushing one piece of chalk into smaller pieces?
In the experiment with chalk (CaCO3) and hydrochloric acid (HCl), what is the purpose of crushing one piece of chalk into smaller pieces?
Why do reactions between covalent molecules tend to be slower compared to reactions involving ions in aqueous solutions?
Why do reactions between covalent molecules tend to be slower compared to reactions involving ions in aqueous solutions?
Based on the provided text, which of the following best explains how catalysts increase reaction rates?
Based on the provided text, which of the following best explains how catalysts increase reaction rates?
Which of the following experimental procedures described in the material is designed to investigate the effect of concentration on reaction rate?
Which of the following experimental procedures described in the material is designed to investigate the effect of concentration on reaction rate?
When studying the effect of temperature on the reaction rate of potassium permanganate and oxalic acid, why is it important to measure the time for the purple color to disappear?
When studying the effect of temperature on the reaction rate of potassium permanganate and oxalic acid, why is it important to measure the time for the purple color to disappear?
According to the provided text, how does the surface area of a solid reactant affect the reaction rate, and why?
According to the provided text, how does the surface area of a solid reactant affect the reaction rate, and why?
In the context of the experiments described, what is the most likely reason for repeating the measurements multiple times (e.g., three times) when observing the effect of temperature on reaction rate?
In the context of the experiments described, what is the most likely reason for repeating the measurements multiple times (e.g., three times) when observing the effect of temperature on reaction rate?
Consider the reaction: $aA + bB \rightarrow cC + dD$. According to the material, what does the equilibrium constant, K, represent?
Consider the reaction: $aA + bB \rightarrow cC + dD$. According to the material, what does the equilibrium constant, K, represent?
Based on the provided text, predict how the rate of a reaction between two gases will change if the partial pressure of one of the reactants is doubled, assuming all other factors remain constant.
Based on the provided text, predict how the rate of a reaction between two gases will change if the partial pressure of one of the reactants is doubled, assuming all other factors remain constant.
Why is the use of equal amounts of reactants important when investigating the effect of concentration on the rate of reaction between zinc and hydrochloric acid?
Why is the use of equal amounts of reactants important when investigating the effect of concentration on the rate of reaction between zinc and hydrochloric acid?
What is the relationship between the rate of a reaction and its equilibrium constant, based on the provided objectives?
What is the relationship between the rate of a reaction and its equilibrium constant, based on the provided objectives?
The material discusses the reaction of hydrogen peroxide (H2O2) in the presence of manganese dioxide (MnO2). If the reaction proceeds via the following elementary steps:
- $H_2O_2(aq) + MnO_2(s) \longrightarrow H_2O(l) + O_2(g) + MnO(s)$
- $H_2O_2(aq) + MnO(s) \longrightarrow H_2O(l) + MnO_2(s)$
What role does $MnO_2$ play in this reaction?
The material discusses the reaction of hydrogen peroxide (H2O2) in the presence of manganese dioxide (MnO2). If the reaction proceeds via the following elementary steps:
- $H_2O_2(aq) + MnO_2(s) \longrightarrow H_2O(l) + O_2(g) + MnO(s)$
- $H_2O_2(aq) + MnO(s) \longrightarrow H_2O(l) + MnO_2(s)$
What role does $MnO_2$ play in this reaction?
Consider a reaction where the rate doubles for every 10°C increase in temperature. If the reaction takes 60 minutes to complete at 25°C, approximately how long will it take to complete at 45°C?
Consider a reaction where the rate doubles for every 10°C increase in temperature. If the reaction takes 60 minutes to complete at 25°C, approximately how long will it take to complete at 45°C?
In the reaction between oxalic acid and potassium permanganate, the reaction rate dependence on temperature can be modeled using the Arrhenius equation: $k = Ae^{-E_a/RT}$,
where:
- k is the rate constant,
- A is the pre-exponential factor,
- $E_a$ is the activation energy,
- R is the ideal gas constant,
- T is the absolute temperature.
If increasing the temperature from 20°C to 30°C causes the rate constant (k) to double, what can be inferred about the activation energy ($E_a$) for this reaction?
In the reaction between oxalic acid and potassium permanganate, the reaction rate dependence on temperature can be modeled using the Arrhenius equation: $k = Ae^{-E_a/RT}$, where:
- k is the rate constant,
- A is the pre-exponential factor,
- $E_a$ is the activation energy,
- R is the ideal gas constant,
- T is the absolute temperature.
If increasing the temperature from 20°C to 30°C causes the rate constant (k) to double, what can be inferred about the activation energy ($E_a$) for this reaction?
Considering the experimental procedure involving chalk and hydrochloric acid, which of the following modifications would most effectively demonstrate the combined effects of both surface area and concentration on reaction rate?
Considering the experimental procedure involving chalk and hydrochloric acid, which of the following modifications would most effectively demonstrate the combined effects of both surface area and concentration on reaction rate?
Given two reactions: one involving aqueous ions (Reaction A) and another involving covalent molecules (Reaction B). Reaction A occurs almost instantaneously at room temperature, while Reaction B requires significant heating to proceed at a noticeable rate. Which statement provides the MOST accurate comparison of the activation energies ($E_a$) for these two reactions?
Given two reactions: one involving aqueous ions (Reaction A) and another involving covalent molecules (Reaction B). Reaction A occurs almost instantaneously at room temperature, while Reaction B requires significant heating to proceed at a noticeable rate. Which statement provides the MOST accurate comparison of the activation energies ($E_a$) for these two reactions?
A chemist performs the hydrogen peroxide decomposition experiment and observes the following: Beaker 1 (no catalyst): Very slow bubbling. Beaker 2 (with manganese dioxide): Vigorous bubbling. The chemist then filters the contents of Beaker 2 to remove the manganese dioxide, and adds the filtered solution to Beaker 1. What is the MOST likely observation, and what conclusion can be drawn?
A chemist performs the hydrogen peroxide decomposition experiment and observes the following: Beaker 1 (no catalyst): Very slow bubbling. Beaker 2 (with manganese dioxide): Vigorous bubbling. The chemist then filters the contents of Beaker 2 to remove the manganese dioxide, and adds the filtered solution to Beaker 1. What is the MOST likely observation, and what conclusion can be drawn?
Imagine a scenario where the chalk experiment is conducted inside a sealed container connected to a pressure sensor. Initially, a large piece of chalk and crushed chalk are placed in separate compartments within the container, each exposed to the same amount of hydrochloric acid once the experiment begins. Which of the following pressure curves would most accurately depict the change in pressure over time for both reactions, assuming temperature is constant?
Imagine a scenario where the chalk experiment is conducted inside a sealed container connected to a pressure sensor. Initially, a large piece of chalk and crushed chalk are placed in separate compartments within the container, each exposed to the same amount of hydrochloric acid once the experiment begins. Which of the following pressure curves would most accurately depict the change in pressure over time for both reactions, assuming temperature is constant?
A researcher is studying the catalyzed decomposition of hydrogen peroxide using manganese dioxide ($MnO_2$). They perform the reaction under two different sets of conditions:
- Condition A: Standard conditions, using pure $MnO_2$ as the catalyst.
- Condition B: $MnO_2$ is mixed with a fine powder of an inert substance that does not participate in the reaction but reduces the effective surface area of the catalyst.
Assuming all other variables are kept constant, how would the activation energy ($E_a$) and the initial rate of the reaction differ between the two conditions, if at all?
A researcher is studying the catalyzed decomposition of hydrogen peroxide using manganese dioxide ($MnO_2$). They perform the reaction under two different sets of conditions:
- Condition A: Standard conditions, using pure $MnO_2$ as the catalyst.
- Condition B: $MnO_2$ is mixed with a fine powder of an inert substance that does not participate in the reaction but reduces the effective surface area of the catalyst.
Assuming all other variables are kept constant, how would the activation energy ($E_a$) and the initial rate of the reaction differ between the two conditions, if at all?
A laboratory student accidentally mixes the oxalic acid with the hydrochloric acid before adding the potassium permanganate. How would you expect this to affect the observed results in comparison to the standard procedure, and why?
A laboratory student accidentally mixes the oxalic acid with the hydrochloric acid before adding the potassium permanganate. How would you expect this to affect the observed results in comparison to the standard procedure, and why?
During the hydrogen peroxide decomposition with manganese dioxide, a student observes that upon adding manganese dioxide, there's a significant temperature increase in the solution. Based on this observation, which of the following statements is most accurate?
During the hydrogen peroxide decomposition with manganese dioxide, a student observes that upon adding manganese dioxide, there's a significant temperature increase in the solution. Based on this observation, which of the following statements is most accurate?
In the context of chemical kinetics, what is the physical significance of the pre-exponential factor (A) in the Arrhenius equation ($k = Ae^{-E_a/RT}$)?
In the context of chemical kinetics, what is the physical significance of the pre-exponential factor (A) in the Arrhenius equation ($k = Ae^{-E_a/RT}$)?
A chemist is studying the kinetics of a reaction and finds that the addition of a small amount of a certain substance dramatically increases the reaction rate, but the substance is not consumed during the reaction. However, upon closer inspection, the chemist discovers that the substance reacts with one of the intermediate products, forming a different, more stable intermediate. How does this affect the overall reaction pathway?
A chemist is studying the kinetics of a reaction and finds that the addition of a small amount of a certain substance dramatically increases the reaction rate, but the substance is not consumed during the reaction. However, upon closer inspection, the chemist discovers that the substance reacts with one of the intermediate products, forming a different, more stable intermediate. How does this affect the overall reaction pathway?
Suppose a researcher discovers that the rate of a particular reaction decreases with increasing temperature. Which of the following conclusions is most likely to be valid regarding this reaction?
Suppose a researcher discovers that the rate of a particular reaction decreases with increasing temperature. Which of the following conclusions is most likely to be valid regarding this reaction?
Imagine a scenario where the hydrogen peroxide decomposition experiment is performed using manganese dioxide ($MnO_2$) immobilized on the surface of a porous material. Over time, it's observed that the reaction rate decreases significantly, even though the concentration of hydrogen peroxide remains high. Which of the following is the MOST plausible explanation for this decrease in reaction rate?
Imagine a scenario where the hydrogen peroxide decomposition experiment is performed using manganese dioxide ($MnO_2$) immobilized on the surface of a porous material. Over time, it's observed that the reaction rate decreases significantly, even though the concentration of hydrogen peroxide remains high. Which of the following is the MOST plausible explanation for this decrease in reaction rate?
A chemist is investigating the effect of a potential catalyst on a reaction. They run the reaction with and without the catalyst and measure the rate constants at different temperatures. They find that the catalyzed reaction has a lower activation energy ($E_a$) but also a significantly lower pre-exponential factor (A) compared to the uncatalyzed reaction. Under what conditions, if any, would the catalyzed reaction be slower than the uncatalyzed reaction?
A chemist is investigating the effect of a potential catalyst on a reaction. They run the reaction with and without the catalyst and measure the rate constants at different temperatures. They find that the catalyzed reaction has a lower activation energy ($E_a$) but also a significantly lower pre-exponential factor (A) compared to the uncatalyzed reaction. Under what conditions, if any, would the catalyzed reaction be slower than the uncatalyzed reaction?
A researcher performs the chalk and hydrochloric acid experiment and accurately measures the initial rate of carbon dioxide production for both the large chalk piece and the crushed chalk. After analyzing the data, they observe that the initial rate for the crushed chalk is significantly higher, but the total amount of carbon dioxide produced is the same for both. They claim that this experiment conclusively proves that increasing surface area increases the rate constant, k, of the reaction. Is their conclusion valid, and why?
A researcher performs the chalk and hydrochloric acid experiment and accurately measures the initial rate of carbon dioxide production for both the large chalk piece and the crushed chalk. After analyzing the data, they observe that the initial rate for the crushed chalk is significantly higher, but the total amount of carbon dioxide produced is the same for both. They claim that this experiment conclusively proves that increasing surface area increases the rate constant, k, of the reaction. Is their conclusion valid, and why?
In a variation to the hydrogen peroxide decomposition experiment, a student uses iron(III) chloride ($FeCl_3$) as a catalyst instead of manganese dioxide ($MnO_2$). They measure the reaction rate at different concentrations of $FeCl_3$ and observe that the reaction rate increases linearly with the concentration of $FeCl_3$ up to a certain point, after which it plateaus and remains constant despite further increases in $FeCl_3$ concentration. Which of the following is the MOST likely explanation for this observation?
In a variation to the hydrogen peroxide decomposition experiment, a student uses iron(III) chloride ($FeCl_3$) as a catalyst instead of manganese dioxide ($MnO_2$). They measure the reaction rate at different concentrations of $FeCl_3$ and observe that the reaction rate increases linearly with the concentration of $FeCl_3$ up to a certain point, after which it plateaus and remains constant despite further increases in $FeCl_3$ concentration. Which of the following is the MOST likely explanation for this observation?
What is the primary focus of the experiment described in the text?
What is the primary focus of the experiment described in the text?
Which of the following is NOT identified as a factor that affects reaction rates?
Which of the following is NOT identified as a factor that affects reaction rates?
What happens to the reaction rate when the concentration of reactants is increased?
What happens to the reaction rate when the concentration of reactants is increased?
What is the approximate effect of increasing the temperature by 10°C on the reaction rate?
What is the approximate effect of increasing the temperature by 10°C on the reaction rate?
What is the role of a catalyst in a chemical reaction, as described in the text?
What is the role of a catalyst in a chemical reaction, as described in the text?
Which of the following is an example of a catalyst used in one of the described procedures?
Which of the following is an example of a catalyst used in one of the described procedures?
What is the purpose of crushing chalk in the experiment with hydrochloric acid?
What is the purpose of crushing chalk in the experiment with hydrochloric acid?
Which type of reaction tends to be faster, according to the text?
Which type of reaction tends to be faster, according to the text?
In the experiment with potassium permanganate and oxalic acid, what indicates the reaction is complete?
In the experiment with potassium permanganate and oxalic acid, what indicates the reaction is complete?
What piece of equipment is used to measure the reaction time in seconds?
What piece of equipment is used to measure the reaction time in seconds?
What is the chemical formula for hydrogen peroxide?
What is the chemical formula for hydrogen peroxide?
What is the chemical formula for chalk?
What is the chemical formula for chalk?
Which acid is used in the experiment with chalk?
Which acid is used in the experiment with chalk?
What is the concentration of the potassium permanganate solution used in the temperature experiment?
What is the concentration of the potassium permanganate solution used in the temperature experiment?
What observation is made when manganese dioxide is added to hydrogen peroxide?
What observation is made when manganese dioxide is added to hydrogen peroxide?
In the equilibrium expression $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$, what do the square brackets represent?
In the equilibrium expression $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$, what do the square brackets represent?
In the equilibrium expression $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$, what do the lowercase letters a, b, c, and d represent?
In the equilibrium expression $K = \frac{[C]^c[D]^d}{[A]^a[B]^b}$, what do the lowercase letters a, b, c, and d represent?
Which piece of lab equipment is used to hold small amounts of reactants in the procedures?
Which piece of lab equipment is used to hold small amounts of reactants in the procedures?
What is the concentration of hydrochloric acid used in the concentration experiment?
What is the concentration of hydrochloric acid used in the concentration experiment?
Which reactant is used in the experiment to observe the effect of temperature?
Which reactant is used in the experiment to observe the effect of temperature?
What piece of equipment is used to deliver drops of solutions?
What piece of equipment is used to deliver drops of solutions?
Which of the following is NOT a material needed for the experiments?
Which of the following is NOT a material needed for the experiments?
According to the theory, what is required for reactant molecules to react?
According to the theory, what is required for reactant molecules to react?
Based on the procedures, what needs to be added to the well after filling it with hydrogen peroxide?
Based on the procedures, what needs to be added to the well after filling it with hydrogen peroxide?
Which of the following does not directly appear as a material in the experiment?
Which of the following does not directly appear as a material in the experiment?
What is the role of hydrogen peroxide in the catalyst experiment?
What is the role of hydrogen peroxide in the catalyst experiment?
What type of reaction uses warmed saturated oxalic acid?
What type of reaction uses warmed saturated oxalic acid?
What is initially deep purple in the temperature experiment?
What is initially deep purple in the temperature experiment?
What is added to the wells filled with warmed saturated oxalic acid?
What is added to the wells filled with warmed saturated oxalic acid?
What needs to be measured in order to understand the effect of temperature in the procedure?
What needs to be measured in order to understand the effect of temperature in the procedure?
How many times should the measurement be repeated to identify the temperature effect?
How many times should the measurement be repeated to identify the temperature effect?
How should the wells be filled with oxalic acid?
How should the wells be filled with oxalic acid?
What is the state of the oxalic acid used in the temperature experiment?
What is the state of the oxalic acid used in the temperature experiment?
Which equation represents the reaction for the effect of temperature experiment?
Which equation represents the reaction for the effect of temperature experiment?
How do covalent molecules impact the reaction rate?
How do covalent molecules impact the reaction rate?
What is compared after placing equal amounts of zinc pieces into two small test tubes?
What is compared after placing equal amounts of zinc pieces into two small test tubes?
What amount of 6 M HCl is added to the zinc pieces for the concentration experiment?
What amount of 6 M HCl is added to the zinc pieces for the concentration experiment?
What is observed and compared after placing chalk pieces in the well plate?
What is observed and compared after placing chalk pieces in the well plate?
For solids, what determines the reaction rate?
For solids, what determines the reaction rate?
Flashcards
Reaction Rate
Reaction Rate
The change in the concentration of a reactant or product per unit time.
Collision Theory
Collision Theory
Reactions need molecules to collide with proper orientation and sufficient energy.
Reaction Rate of Aqueous Ions
Reaction Rate of Aqueous Ions
Ions in aqueous solutions react very quickly due to their mobility and charge.
Reaction Rate of Covalent Molecules
Reaction Rate of Covalent Molecules
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Surface Area and Reaction Rate
Surface Area and Reaction Rate
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Concentration Effect on Reaction Rate
Concentration Effect on Reaction Rate
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Temperature Effect on Reaction Rate
Temperature Effect on Reaction Rate
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Catalyst
Catalyst
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How Catalysts Work
How Catalysts Work
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HCl Concentration Effect
HCl Concentration Effect
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Decomposition of H2O2
Decomposition of H2O2
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Objectives of the experiment
Objectives of the experiment
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Aqueous ion reaction rates
Aqueous ion reaction rates
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Covalent molecule reactions
Covalent molecule reactions
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Surface area
Surface area
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Concentration and Reaction Rate
Concentration and Reaction Rate
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Temperature Effect
Temperature Effect
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Catalysts effect on activation energy
Catalysts effect on activation energy
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Equilibrium Constant
Equilibrium Constant
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Crushed Chalk and HCl Reaction
Crushed Chalk and HCl Reaction
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Effect of Higher HCl Concentration
Effect of Higher HCl Concentration
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Hydrogen Peroxide Decomposition
Hydrogen Peroxide Decomposition
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Manganese Dioxide Catalyst
Manganese Dioxide Catalyst
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Study Notes
- The lab activity aims to experimentally determine how the nature of reactants, reactant concentration, temperature, and catalyst presence impact reaction rates.
- The lab also aims to understand the relationship between reaction rate and equilibrium constant.
Materials Needed
- CaCO3 (chalk)
- 12 well plate
- 6M HCl
- 3 M HCl
- Test tubes
- Zinc Pieces
- Manganese dioxide
- Hydrogen peroxide
- Oxalic acid
- 0.10 M KMnO4
- Dropper
- Toothpick
Reaction Rate Definition
- The rate of a chemical reaction refers to the change in reactant or product concentration per unit time.
Conditions for Reaction
- Reactions require reactant molecules to collide with proper orientation and energy at or above the activation energy.
Factors Affecting Reaction Rates
- The nature of the reactants
- Concentration
- Temperature
- Catalyst
Nature of Reactants
- Reaction rates can vary based on the nature of the reactants
- Reactions involving ions in aqueous solution tend to be extremely fast.
- Reactions involving covalent molecules tend to be slow due to the need to break covalent bonds, which require higher activation energies.
- For solid reactants, the surface area affects the reaction rate, with greater surface area leading to faster reactions.
- A flat smooth piece of iron will rust slower than iron fillings as an example.
Concentration
- The reaction rate typically increases with an increase in reactant concentration.
Temperature
- As a rule of thumb, the reaction rate doubles for every 10°C rise in temperature.
Catalyst
- A catalyst increases the reaction rate without being consumed in the reaction and lowers the activation energy required for a reactive molecular collision, often by providing a surface for the reactants to meet.
Equilibrium Expression
- For a reaction aA + bB → cC + dD, the equilibrium expression is given by: K = ([C]^c[D]^d) / ([A]^a[B]^b)
Procedure: Nature of Reactants
- Two small chalk pieces (CaCO3) of similar size are used.
- One piece is placed in a well of a 12-well plate, while the other is crushed into small pieces and placed in a second well.
- Equal amounts of dilute hydrochloric acid are added to each well.
- The rate of carbon dioxide evolution is observed and compared.
- Repeat if results are not conclusive
Procedure: Concentration
- Equal amounts of zinc pieces are placed into two test tubes.
- 2 mL of 6 M HCl is added to one tube, and 2 mL of 3 M HCl is added to the other and the reaction rates are compared.
Procedure: Effect of Temperature
- The effect of temperature is determined by observing the reduction of potassium permanganate by oxalic acid, according to reaction: 3H2C2O4 + 2KMnO4 → 6CO2 + 2KOH + 2H2O + 2MnO2.
- The permanganate ion (MnO4) is deep purple, with the completion of the reaction indicated by the disappearance of this color.
- Three wells are filled one-half full with warmed saturated oxalic acid, adding 3 drops of 0.10 M KMnO4 solution to the first well, and measuring the time for the purple color to disappear, repeating 2 more times.
- The process is repeated with three wells filled one-half full with room temperature saturated oxalic acid, adding 3 drops of 0.10 M KMnO4 solution to the first well, and measuring the time required for the purple color to disappear, repeating 2 more times.
- Record all the reaction times.
Procedure: Effect of Catalysts
- Hydrogen peroxide slowly decomposes at room temperature.
- A well in a microplate is filled one-half full with hydrogen peroxide, observing it.
- A few grains of manganese dioxide are added and observed.
- Record all observations
Lab Observation Recording
- Nature of Reactants
- Reactants: Large chalk piece + HCl, Crushed chalk piece + HCl
- Concentration
- Reactants: Zn + 6M HCl, Zn + 3M HCl
- Temperature
- Warmed oxalic acid reaction times
- Room temperature oxalic acid reaction times
- Catalysts
- Reactants: H2O2, H2O2 + MnO2
Guide Questions
- What does the reaction of chalk with HCl show about reaction rates?
- Should the reaction rate change if the size of the Zn pieces changes? Why or why not?
- When the concentration of HCl is increased, what happens to the reaction rate? Is this what you expected? and Why or why not?
- What effect does temperature have on the reaction rate of oxalic acid and permanganate?
- What effect does MnO2 have on the reaction rate of the decomposition of hydrogen peroxide?
- Does adding a catalyst to a given reaction shift the equilibrium so that more product is produced?
- What is the main purpose of a catalyst?
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