Podcast
Questions and Answers
Which factor does NOT directly influence the reaction rate of a chemical reaction?
Which factor does NOT directly influence the reaction rate of a chemical reaction?
- The presence of a catalyst
- The concentration of reactants
- The color of the reaction vessel (correct)
- The nature of the reactants involved
How does increasing the concentration of reactants generally affect the rate of a chemical reaction?
How does increasing the concentration of reactants generally affect the rate of a chemical reaction?
- It has no effect on the reaction rate.
- It increases the reaction rate. (correct)
- It decreases the reaction rate.
- It stops the reaction completely.
According to the rate law, rate = k[A], what happens to the reaction rate if the concentration of A is doubled in a first-order reaction?
According to the rate law, rate = k[A], what happens to the reaction rate if the concentration of A is doubled in a first-order reaction?
- The reaction rate is halved.
- The reaction rate remains the same.
- The reaction rate is quadrupled.
- The reaction rate is doubled. (correct)
For gaseous reactants, how does increasing the pressure generally affect the reaction rate?
For gaseous reactants, how does increasing the pressure generally affect the reaction rate?
Why does increasing the surface area of a solid reactant increase the reaction rate?
Why does increasing the surface area of a solid reactant increase the reaction rate?
What is the primary mechanism by which a catalyst increases the rate of a chemical reaction?
What is the primary mechanism by which a catalyst increases the rate of a chemical reaction?
How does increasing the temperature affect the rate constant (k) and the overall reaction rate?
How does increasing the temperature affect the rate constant (k) and the overall reaction rate?
In the reaction of hydroxide with tribromide ion, what is the effect of increasing the tribromide ion concentration on the reaction rate and the rate constant (k)?
In the reaction of hydroxide with tribromide ion, what is the effect of increasing the tribromide ion concentration on the reaction rate and the rate constant (k)?
If water is added to the reaction of hydroxide with tribromide ion, increasing the volume, how is the reaction rate affected?
If water is added to the reaction of hydroxide with tribromide ion, increasing the volume, how is the reaction rate affected?
What effect does decreasing the pH of a solution have on the reaction rate of a reaction involving hydroxide ions?
What effect does decreasing the pH of a solution have on the reaction rate of a reaction involving hydroxide ions?
How does increasing the pH of a solution affect the reaction rate of a reaction that involves hydroxide ions?
How does increasing the pH of a solution affect the reaction rate of a reaction that involves hydroxide ions?
Which of the following is NOT a direct way to increase the reaction rate for a reaction involving solid reactants?
Which of the following is NOT a direct way to increase the reaction rate for a reaction involving solid reactants?
For the reaction of hydroxide with tribromide ion, what is the effect of using a catalyst that lowers the activation energy by 50%?
For the reaction of hydroxide with tribromide ion, what is the effect of using a catalyst that lowers the activation energy by 50%?
Consider a reaction where both H+ and OH- ions play a role. How would a significant increase in both acidic and basic conditions simultaneously affect this reaction?
Consider a reaction where both H+ and OH- ions play a role. How would a significant increase in both acidic and basic conditions simultaneously affect this reaction?
In a scenario where a reversible reaction is at equilibrium, what is the effect of adding a catalyst?
In a scenario where a reversible reaction is at equilibrium, what is the effect of adding a catalyst?
How does increasing the surface area of a solid reactant affect the activation energy of a reaction?
How does increasing the surface area of a solid reactant affect the activation energy of a reaction?
Consider a reaction that releases heat (exothermic). What would be the effect of significantly lowering the temperature on both the reaction rate and the equilibrium?
Consider a reaction that releases heat (exothermic). What would be the effect of significantly lowering the temperature on both the reaction rate and the equilibrium?
Which statement accurately describes the impact of reactant concentration on the rate constant (k) and the reaction rate?
Which statement accurately describes the impact of reactant concentration on the rate constant (k) and the reaction rate?
How does the presence of a catalyst in a reversible reaction affect the equilibrium constant (K)?
How does the presence of a catalyst in a reversible reaction affect the equilibrium constant (K)?
What is the effect of increasing the temperature on the equilibrium constant (K) of an endothermic reaction?
What is the effect of increasing the temperature on the equilibrium constant (K) of an endothermic reaction?
How does decreasing the volume of a reaction system containing gaseous reactants affect the reaction rate?
How does decreasing the volume of a reaction system containing gaseous reactants affect the reaction rate?
If a reaction proceeds via a multi-step mechanism, what effect would a catalyst have on the rate-determining step?
If a reaction proceeds via a multi-step mechanism, what effect would a catalyst have on the rate-determining step?
Consider a scenario where a reaction is diffusion-controlled. How would increasing the viscosity of the solvent affect the reaction rate?
Consider a scenario where a reaction is diffusion-controlled. How would increasing the viscosity of the solvent affect the reaction rate?
In the reaction of hydroxide with tribromide ion, if the initial concentration of hydroxide ions is significantly higher than that of tribromide ions, how would further increases in hydroxide concentration affect the reaction rate?
In the reaction of hydroxide with tribromide ion, if the initial concentration of hydroxide ions is significantly higher than that of tribromide ions, how would further increases in hydroxide concentration affect the reaction rate?
How does the ionic strength of a solution affect the rate of a reaction between ions of the same charge?
How does the ionic strength of a solution affect the rate of a reaction between ions of the same charge?
For a reaction with a complex rate law involving multiple reactants, how would you determine the effect of a catalyst on each individual step of the mechanism?
For a reaction with a complex rate law involving multiple reactants, how would you determine the effect of a catalyst on each individual step of the mechanism?
If the rate of a reaction doubles for every 10C increase in temperature, what is this an example of?
If the rate of a reaction doubles for every 10C increase in temperature, what is this an example of?
How does the addition of an inert gas at constant volume affect the reaction rate of a gas-phase reaction?
How does the addition of an inert gas at constant volume affect the reaction rate of a gas-phase reaction?
For a zero-order reaction, how does changing the concentration of the reactants affect the reaction rate?
For a zero-order reaction, how does changing the concentration of the reactants affect the reaction rate?
Consider the gas-phase reaction $2NO(g) + O_2(g)
ightarrow 2NO_2(g)$. Which change will increase the rate of the reaction?
Consider the gas-phase reaction $2NO(g) + O_2(g) ightarrow 2NO_2(g)$. Which change will increase the rate of the reaction?
Which of the following scenarios would result in an increase in the rate constant, k?
Which of the following scenarios would result in an increase in the rate constant, k?
In the elementary reaction $A + B
ightarrow C$, if the concentrations of both A and B are doubled, by what factor does the reaction rate increase?
In the elementary reaction $A + B ightarrow C$, if the concentrations of both A and B are doubled, by what factor does the reaction rate increase?
A reaction is found to be zero order in reactant A. Which of the following statements is true?
A reaction is found to be zero order in reactant A. Which of the following statements is true?
The reaction $A + B
ightarrow products$ has the rate law Rate = $k[A]^2[B]$. If the concentration of A is doubled and the concentration of B is halved, what happens to the reaction rate?
The reaction $A + B ightarrow products$ has the rate law Rate = $k[A]^2[B]$. If the concentration of A is doubled and the concentration of B is halved, what happens to the reaction rate?
Consider a complex reaction with multiple steps. The activation energy for the first step is high, while that of other steps is considerably low. What can be inferred?
Consider a complex reaction with multiple steps. The activation energy for the first step is high, while that of other steps is considerably low. What can be inferred?
The rate constant, k, for a reaction is determined to be $4.3 \times 10^{-4} s^{-1}$ at 25C and $8.6 \times 10^{-4} s^{-1}$ at 35C. What does this imply about the reaction?
The rate constant, k, for a reaction is determined to be $4.3 \times 10^{-4} s^{-1}$ at 25C and $8.6 \times 10^{-4} s^{-1}$ at 35C. What does this imply about the reaction?
For a reaction where the rate law is Rate = k[A][B], under what conditions would you expect the reaction to appear pseudo-first order?
For a reaction where the rate law is Rate = k[A][B], under what conditions would you expect the reaction to appear pseudo-first order?
Why might a theoretical reaction rate calculated using collision theory differ significantly from the experimentally observed rate?
Why might a theoretical reaction rate calculated using collision theory differ significantly from the experimentally observed rate?
Imagine a reaction where the products themselves act as catalysts (autocatalysis). What would the rate of reaction look like over time?
Imagine a reaction where the products themselves act as catalysts (autocatalysis). What would the rate of reaction look like over time?
Consider a reaction where the rate is pressure dependent. If the system volume is suddenly doubled, and the reaction is first order, what happens to the initial reaction rate?
Consider a reaction where the rate is pressure dependent. If the system volume is suddenly doubled, and the reaction is first order, what happens to the initial reaction rate?
Which statement best describes the effect of the nature of reactants on reaction rate?
Which statement best describes the effect of the nature of reactants on reaction rate?
Consider a reaction where the rate increases proportionally with the concentration of reactant A. Which of the following rate laws is most likely to describe this reaction?
Consider a reaction where the rate increases proportionally with the concentration of reactant A. Which of the following rate laws is most likely to describe this reaction?
For the Haber process ($N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$), how does increasing the total pressure of the system typically affect the reaction rate?
For the Haber process ($N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$), how does increasing the total pressure of the system typically affect the reaction rate?
Why does powdered zinc react more rapidly with hydrochloric acid than a single piece of zinc of the same mass?
Why does powdered zinc react more rapidly with hydrochloric acid than a single piece of zinc of the same mass?
A catalyst is added to a reaction. Which of the following is the primary effect of the catalyst on the reaction?
A catalyst is added to a reaction. Which of the following is the primary effect of the catalyst on the reaction?
According to collision theory, why does increasing temperature generally increase the rate of a chemical reaction?
According to collision theory, why does increasing temperature generally increase the rate of a chemical reaction?
In the context of a reaction involving tribromide ions ($Br_3^-$) and hydroxide ions ($OH^-$), what happens to the reaction rate if the concentration of $Br_3^-$ is doubled?
In the context of a reaction involving tribromide ions ($Br_3^-$) and hydroxide ions ($OH^-$), what happens to the reaction rate if the concentration of $Br_3^-$ is doubled?
If water is added to the reaction ($OH^- + Br_3^- \rightarrow HOBr + 2Br^-$), thereby increasing the volume of the solution, how does this affect the rate constant (k)?
If water is added to the reaction ($OH^- + Br_3^- \rightarrow HOBr + 2Br^-$), thereby increasing the volume of the solution, how does this affect the rate constant (k)?
For a reaction that consumes hydroxide ions ($OH^-$), what is the effect of decreasing the pH of the solution on the reaction rate?
For a reaction that consumes hydroxide ions ($OH^-$), what is the effect of decreasing the pH of the solution on the reaction rate?
For a reaction involving a solid reactant, which of the following actions would NOT typically increase the reaction rate?
For a reaction involving a solid reactant, which of the following actions would NOT typically increase the reaction rate?
Consider a reaction with a significantly high activation energy. What would be the effect of introducing a catalyst on the reaction rate?
Consider a reaction with a significantly high activation energy. What would be the effect of introducing a catalyst on the reaction rate?
In a reversible reaction at equilibrium, what effect does the addition of a catalyst have on the equilibrium concentrations of reactants and products?
In a reversible reaction at equilibrium, what effect does the addition of a catalyst have on the equilibrium concentrations of reactants and products?
A reaction is carried out in both a small flask and a large beaker, but all other conditions are identical. Which container will likely have a faster reaction rate, and why?
A reaction is carried out in both a small flask and a large beaker, but all other conditions are identical. Which container will likely have a faster reaction rate, and why?
Most reactions speed up when the temperature increases. Which statement explains why?
Most reactions speed up when the temperature increases. Which statement explains why?
Consider a reaction with the rate law $rate = k[A]^2[B]$. If the concentration of A is halved and the concentration of B is doubled, what is the effect on the reaction rate?
Consider a reaction with the rate law $rate = k[A]^2[B]$. If the concentration of A is halved and the concentration of B is doubled, what is the effect on the reaction rate?
For an endothermic reaction, how does increasing the temperature typically affect the equilibrium constant (K)?
For an endothermic reaction, how does increasing the temperature typically affect the equilibrium constant (K)?
For a gas-phase reaction, how does decreasing the volume of the reaction vessel affect the reaction rate?
For a gas-phase reaction, how does decreasing the volume of the reaction vessel affect the reaction rate?
In a multi-step reaction mechanism, what specific effect does a catalyst have, and on which step does it exert this effect?
In a multi-step reaction mechanism, what specific effect does a catalyst have, and on which step does it exert this effect?
Consider a reaction in a highly viscous solvent. How would increasing the viscosity likely affect the reaction rate, assuming the reaction is diffusion-controlled?
Consider a reaction in a highly viscous solvent. How would increasing the viscosity likely affect the reaction rate, assuming the reaction is diffusion-controlled?
Consider the reaction: $OH^- + Br_3^- \rightarrow products$. If the concentration of $OH^-$ is significantly higher than that of $Br_3^-$, how would further increases in $OH^-$ concentration affect the reaction rate?
Consider the reaction: $OH^- + Br_3^- \rightarrow products$. If the concentration of $OH^-$ is significantly higher than that of $Br_3^-$, how would further increases in $OH^-$ concentration affect the reaction rate?
How might increasing the ionic strength of a solution affect the rate of a reaction between two positively charged ions?
How might increasing the ionic strength of a solution affect the rate of a reaction between two positively charged ions?
Which of the following is the least plausible explanation for why the actual reaction rate might deviate from the predicted rate based solely on collision theory?
Which of the following is the least plausible explanation for why the actual reaction rate might deviate from the predicted rate based solely on collision theory?
At what point does the addition of a catalyst cease to have a significant effect on the rate of a reaction?
At what point does the addition of a catalyst cease to have a significant effect on the rate of a reaction?
What is the effect on the reaction rate if a reactant's concentration is increased tenfold and the reaction is second order with respect to that reactant?
What is the effect on the reaction rate if a reactant's concentration is increased tenfold and the reaction is second order with respect to that reactant?
If the rate of a reaction increases dramatically with only a slight increase in temperature, what does this suggest about the reaction?
If the rate of a reaction increases dramatically with only a slight increase in temperature, what does this suggest about the reaction?
When is the rate constant (k) most accurately described as truly constant?
When is the rate constant (k) most accurately described as truly constant?
For a reaction between two gases, the activation energy is largely dependent on the energy needed to stretch and deform bonds. If the gases are contained in a container with frictionless, perfectly elastic walls (i.e. no energy is lost on collision with the walls), should the reaction rate increase or decrease and why?
For a reaction between two gases, the activation energy is largely dependent on the energy needed to stretch and deform bonds. If the gases are contained in a container with frictionless, perfectly elastic walls (i.e. no energy is lost on collision with the walls), should the reaction rate increase or decrease and why?
How does the presence of an inert gas affect the rate of a liquid-phase reaction?
How does the presence of an inert gas affect the rate of a liquid-phase reaction?
Most reactions proceed faster at high temperatures. However, some reactions can explode instead of simply increasing in rate. The explosion is most likely caused by which of the following?
Most reactions proceed faster at high temperatures. However, some reactions can explode instead of simply increasing in rate. The explosion is most likely caused by which of the following?
If a homogeneous catalyst cannot be separated from the reaction mixture after the reaction is complete, how can its impact on the reaction rate be minimized in subsequent uses of the same reaction vessel?
If a homogeneous catalyst cannot be separated from the reaction mixture after the reaction is complete, how can its impact on the reaction rate be minimized in subsequent uses of the same reaction vessel?
For a zero-order reaction, how does an increase in reactant concentration affect the half-life ($t_{1/2}$)?
For a zero-order reaction, how does an increase in reactant concentration affect the half-life ($t_{1/2}$)?
In what way does the addition of a non-reacting gas to a constant-volume container influence the rate of a gaseous reaction?
In what way does the addition of a non-reacting gas to a constant-volume container influence the rate of a gaseous reaction?
How does reciprocating between a small and a large container influence the rate of a reaction?
How does reciprocating between a small and a large container influence the rate of a reaction?
The addition of a catalyst has what effect on a reaction that is thermodynamically unfavorable?
The addition of a catalyst has what effect on a reaction that is thermodynamically unfavorable?
High-energy radiation can cause the rate of certain reactions to suddenly increase, even at standard temperature and pressure (STP). How does this occur?
High-energy radiation can cause the rate of certain reactions to suddenly increase, even at standard temperature and pressure (STP). How does this occur?
Increasing the ionic strength of a solution can impact the activation energies of ionic reactions. Under which condition(s) does the activation energy increase?
Increasing the ionic strength of a solution can impact the activation energies of ionic reactions. Under which condition(s) does the activation energy increase?
How does strong mixing influence the rate of a reaction with a solid catalyst?
How does strong mixing influence the rate of a reaction with a solid catalyst?
Which of the following is the most influential factor in industrial catalytic reaction design?
Which of the following is the most influential factor in industrial catalytic reaction design?
A dissolved metal catalyst can sometimes be precipitated out of a solution by altering which parameters?
A dissolved metal catalyst can sometimes be precipitated out of a solution by altering which parameters?
Flashcards
Nature of Reactants
Nature of Reactants
Property of reactants affecting how fast a reaction occurs.
Concentration
Concentration
More molecules increase collisions, thus reaction rate .
First-Order Reaction
First-Order Reaction
rate = k[A], rate increases. (k: rate constant, [A]: concentration of A.)
Pressure in Gases
Pressure in Gases
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Surface Atoms
Surface Atoms
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Surface Area
Surface Area
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Catalyst
Catalyst
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Activation Energy
Activation Energy
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Rate Constant (k)
Rate Constant (k)
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Alternative Pathway
Alternative Pathway
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Temperature
Temperature
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Molecular Motion
Molecular Motion
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Concentration & Reaction Rate vs. k
Concentration & Reaction Rate vs. k
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Increasing Volume
Increasing Volume
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Increase Temperature
Increase Temperature
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Decrease Volume
Decrease Volume
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Decreasing pH
Decreasing pH
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How Acid Decreases Rate
How Acid Decreases Rate
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Increasing pH
Increasing pH
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Increased Reactant Concentration
Increased Reactant Concentration
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pH Affects H+ and OH-
pH Affects H+ and OH-
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Reaction Rate
Reaction Rate
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Acid neutralizes hydroxide
Acid neutralizes hydroxide
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Pressure effect on gaseous reaction rate
Pressure effect on gaseous reaction rate
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Study Notes
- Reactant nature affects reaction rate.
Concentration
- More reactant concentration generally speeds up reaction rate, causing more collisions.
- As seen in the rate law (rate = k[A] for a first-order reaction), increasing [A] increases the rate.
Gases
- For gaseous reactants, increased pressure increases reaction rate, similar to increasing concentration and molecular collisions.
Solids
- For solids, reaction is limited to surface atoms.
- Increased surface area increases the reaction rate.
Catalysts
- A catalyst lowers activation energy, increasing the rate constant (k) and reaction rate.
- Catalysts offer a lower activation energy pathway for reactions.
Temperature
- Higher temperatures generally increase the reaction rate.
- Higher temperatures mean more molecular collisions and more energy to break bonds.
Concentration and Volume Changes
- Considering the reaction: OH- + Br3- → HOBr- + 2Br- + H2O (in water).
- Increasing a reactant's concentration (e.g., tri-bromide) increases reaction rate but does not affect the rate constant (k).
- Rate constant (k) is based on activation energy and temperature.
- Adding water (increasing volume) does not change rate constant (k).
- Increasing volume (adding water) decreases the reaction rate by lowering reactant concentrations.
- Decreasing volume (e.g., by evaporation) increases reactant concentrations, increasing the reaction rate.
Temperature and pH Effects
- Increasing temperature increases the rate constant (k), which consequently increases the reaction rate.
- Decreasing pH acidifies the solution, raising H+ concentration.
- Acid + OH- → H2O.
- Increasing H+ (decreasing PH) decreases the concentration of hydroxide (OH-), decreasing the reaction rate if hydroxide is a reactant.
- Increasing pH makes the solution more basic, increasing OH- concentration.
- Increasing OH- concentration (increasing PH) increases the reaction rate, provided hydroxide are a reactant
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