Textbook Question
This graph shows a plot of the rate of a reaction versus the concentration of the reactant.
b. Make a rough sketch of a plot of [A] versus time
Ch.15 - Chemical Kinetics
Chapter 15, Problem 38a
This reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. a. Calculate the rate of the reaction when [N2O5] = 0.055 M
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Identify the order of the reaction with respect to N2O5. Since the reaction is first order in N2O5, the rate law can be expressed as Rate = k[N2O5].
Substitute the given rate constant (k) into the rate law. The rate constant k is given as 0.053/s.
Substitute the concentration of N2O5 into the rate law. The concentration [N2O5] is given as 0.055 M.
Calculate the rate of the reaction by multiplying the rate constant by the concentration of N2O5. Use the formula: Rate = (0.053/s) * (0.055 M).
Express the final rate of the reaction in appropriate units, which in this case would be M/s (molarity per second).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
First-Order Reactions
A first-order reaction is one where the rate of reaction is directly proportional to the concentration of one reactant. In this case, the rate can be expressed as rate = k[N2O5], where k is the rate constant. This means that if the concentration of N2O5 changes, the rate of the reaction will change linearly with it.
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First-Order Reactions
Rate Constant (k)
The rate constant (k) is a proportionality factor that relates the rate of a reaction to the concentration of reactants. It is specific to a given reaction at a particular temperature. In this question, the rate constant is given as 0.053/s, which indicates how quickly the reaction proceeds under the specified conditions.
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Concentration and Rate Calculation
To calculate the rate of a reaction, you multiply the rate constant (k) by the concentration of the reactant. For the given reaction, with [N2O5] at 0.055 M, the rate can be calculated using the formula rate = k[N2O5]. This allows us to determine how fast the reaction is occurring at that specific concentration.
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Related Practice
Textbook Question
This graph shows a plot of the rate of a reaction versus the concentration of the reactant.
c. Write a rate law for the reaction including the value of k.
Textbook Question
What are the units of k for each type of reaction?
a. first-order reaction
b. second-order reaction
c. zero-order reaction
Textbook Question
This reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s. b. What would the rate of the reaction be at the concentration indicated in part a if the reaction were second order? Zero order? (Assume the same numerical value for the rate constant with the appropriate units.)
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Textbook Question
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C. b. What is the overall order of the reaction?
Textbook Question
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if the concentrations of all three reactants are doubled?