Industrial Chemistry - Reaction Order Calculations

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Questions and Answers

What is the order of reaction with respect to reactant B in the given example?

2 (correct)

Given the rate equation: Rate = k[A][B]², what is the overall order of the reaction?

3 (correct)

What is the unit of the rate constant (k) for a third-order reaction?

mol dm⁻³ s⁻¹

s⁻¹

dm³ mol⁻¹ s⁻¹

dm⁶ mol⁻² s⁻¹ (correct)

What is the minimum amount of energy required for a chemical reaction to occur?

Activation energy (C) Signup and view all the answers

What is the term used to describe a collision between reactant particles that results in a chemical reaction?

Effective collision (A) Signup and view all the answers

What is the relationship between the rate constant (k) and the activation energy (Ea) of a reaction?

k is inversely proportional to Ea (A) Signup and view all the answers

What is the significance of the y-intercept in the graph of log(rate) vs log(concentration)?

Rate constant (D) Signup and view all the answers

What is the slope of the graph of log(rate) vs log(concentration)?

Order of reaction (A) Signup and view all the answers

What is the primary use of the Haber Process?

To make chemical fertilizers (C) Signup and view all the answers

What conditions are necessary for the decomposition of hydrogen peroxide with manganese (IV) oxide?

Room temperature and atmospheric pressure (A) Signup and view all the answers

Which catalyst is used in the production of nitric acid?

Platinum alloy (A) Signup and view all the answers

What is the main product obtained from steam reforming of methane?

Syngas (A) Signup and view all the answers

Which process is used for the industrial production of Vitamin C?

Reichstein Process (B) Signup and view all the answers

What is a significant advantage of using a membrane cell over a flowing mercury cell in electrolysis of brine?

Avoids the use of toxic mercury (C) Signup and view all the answers

What is the catalyst employed in the production of methanol?

Copper, Zinc oxide, and Aluminum oxide (B) Signup and view all the answers

Which of the following reactions occurs during the electrolysis of brine at the anode?

2Cl- → Cl2 + 2e- (B) Signup and view all the answers

What is the value of the activation energy (Ea) calculated from the given data?

175.511 kJ mol-1 (D) Signup and view all the answers

What is the correct conversion to Kelvin for a temperature of 25°C?

298 K (C) Signup and view all the answers

What characterizes an activated complex or transition state?

Contains partially broken and formed bonds (A) Signup and view all the answers

Which step in a reaction is referred to as the rate determining step?

The step with the highest activation energy (A) Signup and view all the answers

How does a catalyst affect the activation energy of a reaction?

It lowers the activation energy. (C) Signup and view all the answers

What does the Maxwell-Boltzmann distribution curve represent regarding particle distribution?

The particle energies in two systems with identical areas are the same. (A) Signup and view all the answers

What happens to the activation energy when a catalyst is used in a reaction?

It decreases. (C) Signup and view all the answers

Which statement is true regarding intermediates in a chemical reaction?

They can be isolated. (D) Signup and view all the answers

What effect does an increase in temperature have on kinetic energy and reaction rates?

Increases kinetic energy and accelerates reaction rates. (A) Signup and view all the answers

What is the role of a catalyst in a chemical reaction?

It provides an alternative pathway with lower activation energy. (D) Signup and view all the answers

How does a catalyst affect the equilibrium constant of a reaction?

It has no effect on the equilibrium constant. (A) Signup and view all the answers

What characterizes a heterogeneous catalyst?

It has a different physical state than the reactants. (A) Signup and view all the answers

What happens to a catalyst at the end of a reaction?

It remains chemically unchanged and in the same quantity. (D) Signup and view all the answers

What does the slope of the graph log(rate constant) vs 1/temp represent?

The activation energy divided by the universal gas constant. (A) Signup and view all the answers

Which statement is true regarding negative catalysts?

They increase the activation energy of the reaction. (D) Signup and view all the answers

In the context of catalysts, what does 'k ∝ time' mean?

The rate constant increases over time. (A) Signup and view all the answers

What effect does increasing pressure have on the equilibrium position of a reaction?

It shifts to the right, increasing the percentage yield. (A) Signup and view all the answers

How does higher temperature affect an endothermic reaction?

It favors the forward endothermic reaction. (A) Signup and view all the answers

What is the primary effect of adding a catalyst to a reaction?

It increases the rate of the reaction. (A) Signup and view all the answers

What happens when reactants are added constantly to a reaction at equilibrium?

The equilibrium position shifts to the right. (C) Signup and view all the answers

What is atom economy?

The percentage of reactant atoms turned into products. (A) Signup and view all the answers

What is the main disadvantage of the fermentation process for making ethanoic acid?

The rate of reaction is very slow. (A) Signup and view all the answers

What is the relationship between percentage yield and theoretical yield?

Percentage yield measures completeness of the reaction. (C) Signup and view all the answers

Which principle is associated with Green Chemistry?

Minimizing the use of toxic chemicals. (B) Signup and view all the answers

Study Notes

Industrial Chemistry - Calculations of Reaction Order

Reminder: All reactions are reversible in this chapter; use the reversible symbol (⇌) in chemical equations.
Table: A table shows experiment data, including initial concentrations of reactants A and B, and their corresponding initial reaction rates.

Industrial Chemistry - Rate Constant

Units: The rate of reaction has units of mol dm⁻³ s⁻¹, and the rate constant's unit balances the reaction equation's units to result in mol dm⁻³ s⁻¹.
Zeroth Order: mol dm⁻³ s⁻¹
First Order: s⁻¹
Second Order: dm³ mol⁻¹ s⁻¹
Third Order: dm⁶ mol⁻² s⁻¹

Industrial Chemistry - Graph of log(rate) vs. log(concentration)

Equation: Rate = k[A]^x[B]^y
log (rate) = n log [A] + log k
Slope: Order of reaction
Y-intercept: log(rate constant)
Graph Result: BOTH order of reaction & rate constant from the graph.

Industrial Chemistry - Activation Energy

Definition: The minimum energy required for a chemical reaction to occur.
Effective Collisions: Reactant particles must collide with the correct orientation and energy above the activation energy.
Formula: k = Ae^−Ea/RT, log k₁/k₂ = Ea/(2.3R)[(1/T₁) − (1/T₂)]
Gas Constant(R): 8.314 J K⁻¹ mol⁻¹
Important note: Temperatures in the Arrhenius equation are in Kelvin (K). Convert Celsius to Kelvin by adding 273. Also, the calculation result's unit will be J mol⁻¹ which must be converted to kJ mol⁻¹.

Industrial Chemistry - Energy Profile

Activated Complex/Transition State: Exists at the maximum energy point, containing partially broken and partially formed bonds; highly unstable and cannot be isolated.
Intermediate: Mixture of chemicals between reaction steps, formed between the peaks in the energy profile graph; can be isolated.
Rate Determining Step: The reaction step with the highest activation energy (Ea); typically the first peak in the energy profile.
Catalyst Effect: A catalyst lowers the activation energy, resulting in a lower peak on the energy profile graph.

Industrial Chemistry - Maxwell-Boltzmann Distribution Curve

Area Under Curve: Total number of particles remains the same regardless of temperature.
Kinetic Energy Increase: Increased temperature leads to more particles with kinetic energy greater than the activation energy and increased reaction rate.
Catalyst Effect: With a catalyst, activation energy decreases and more molecules can exceed this energy threshold, further increasing reaction rate.

Industrial Chemistry - Catalyst

Definition: Provides an alternative reaction pathway with lower activation energy.
Unchanged: Remains chemically unchanged throughout the reaction.
Specificity: Catalysts are often specific to a particular reaction.
Effect on Equilibrium: Catalysts affect the rate of both the forward and backward reactions equally, therefore catalysts do not change the equilibrium constant or position.
Homogeneous/Heterogeneous: Homogeneous catalysts share the same physical state as reactants, Heterogeneous catalysts have different physical states.

Industrial Chemistry - Haber Process

Equation: N₂ + 3H₂ ⇌ 2NH₃
Conditions: 450°C and 200 atm with finely divided iron as a catalyst.
Use: Production of ammonia for fertilizer.

Industrial Chemistry - Steam Reforming of Methane

Equation: CH₄ + H₂O ⇌ CO + 3H₂
Conditions: 700-1000°C and 30 atm; endothermic.
Use: Produces syngas (a mixture of CO and H₂); further H₂ can be produced from CO.
Note: Reaction requires heat, but preheating the reactants is used in order to save energy.

Industrial Chemistry - Production of Methanol

Equation: CO + 2H₂ ⇌ CH₃OH
Conditions: 250°C, 50-100 atm, with Cu-ZnO-Al₂O₃ catalyst.
Use: Produces methanol, which can be used to make formaldehyde and acetic acid.

Industrial Chemistry - Production of Nitric Acid

Equations: 4NH₃ + 5O₂ ⇌ 4NO + 6H₂O, 2NO + O₂ ⇌ 2NO₂, 4NO₂ + 2H₂O + O₂⇌ 4HNO₃.
Conditions: 900°C, 8 atm, platinum alloy catalyst.
Use: Producing nitric acid; key in producing fertilizers.

Industrial Chemistry - Reichstein Process (Vitamin C Production)

Equation: Glucose → Sorbitol → Sorbose → KGA → Vitamin C
Note: Natural vitamin C production cannot keep up with demand, therefore the chemical process is necessary to meet supply.

Industrial Chemistry - Electrolysis of Brine

Two Processes:
- Flowing Mercury Cell (Uses Hg): Uses Hg as cathode, with a Na/Hg intermediate produced; the use of Hg is harmful and energy intensive.
- Membrane Cell: Uses a membrane to separate the chlorine and the sodium hydroxide products. This cell is better in terms of safety and energy efficiency.

Industrial Chemistry - Conditions for Optimum Reaction Yields

Pressure: Higher pressures favor reactions with fewer moles of gas on the product side.
Temperature: Endothermic reactions favor higher temps; exothermic reactions favor lower temps.
Catalyst: Accelerates reaction rates without changing equilibrium, thus not affecting yield.
Reactants: Continuously adding reactants shifts equilibrium towards product formation.
Product Removal: Continuously removing products shifts equilibrium towards product.

Industrial Chemistry - Principles of Green Chemistry

Atom Economy: Percentage of reactant atoms converted into desired product.
Less Steps: Fewer steps minimize waste.
Less Toxic Chemicals: Use less harmful/toxic chemicals.
Energy Efficiency: Use catalysts for energy efficiency; renewable resources, etc.
Renewable Materials: Use renewable materials whenever possible.

Industrial Chemistry - Manufacture of Ethanoic Acid

Fermentation: Relatively low-energy process using sugar and yeast. Yield is also low.
Monsanto Process: High-pressure high-temperature process using a rhodium catalyst; high yield; there are also side reactions. A CATIVA process is more efficient, resulting in less waste.

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Test your knowledge on calculating reaction orders in industrial chemistry. This quiz covers topics such as reversible reactions, rate constants, and graphical interpretations of rate versus concentration. Enhance your understanding of how to determine the order of reactions using experimental data and graphical analysis.