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17 Nov 2019
How to do these
Consider a reaction with the stoichiometry A + 2B rightarrow 3D and a rate law: rate = k[A]. The Arrhenius activation energy is 10.0 kJ/mol, and the frequency factor in the Arrhenius equation, A, is 10^13 s^-1. Which of the following changes will increase the rate of the reaction? Increase the activation energy. Increase the [A] Increase the [B] Increase the frequency factor. Only iv Only I ii, iii, and iv i and ii ii and iv Consider the following mechanism for a reaction A rightarrow C Step 1: A + D rightarrow AD Step 2: AD + B rightarrow C + BD Step 3: BD rightarrow B + D Identify any intermediates and catalysts. A reaction is found to have a rate law of Rate = k[B]. The rate constant is determined at a series of temperatures and a plot of ln(k) vs T (T is the temperature in Kelvin) is linear with a slope of -2.0 times 10^3k and an intercept of 25. What is the activation energy and what is the frequency factor (pre-exponential) from an Arrhenius equation analysis?
How to do these
Consider a reaction with the stoichiometry A + 2B rightarrow 3D and a rate law: rate = k[A]. The Arrhenius activation energy is 10.0 kJ/mol, and the frequency factor in the Arrhenius equation, A, is 10^13 s^-1. Which of the following changes will increase the rate of the reaction? Increase the activation energy. Increase the [A] Increase the [B] Increase the frequency factor. Only iv Only I ii, iii, and iv i and ii ii and iv Consider the following mechanism for a reaction A rightarrow C Step 1: A + D rightarrow AD Step 2: AD + B rightarrow C + BD Step 3: BD rightarrow B + D Identify any intermediates and catalysts. A reaction is found to have a rate law of Rate = k[B]. The rate constant is determined at a series of temperatures and a plot of ln(k) vs T (T is the temperature in Kelvin) is linear with a slope of -2.0 times 10^3k and an intercept of 25. What is the activation energy and what is the frequency factor (pre-exponential) from an Arrhenius equation analysis?
Irving HeathcoteLv2
2 Apr 2019