Exam 13: Chemical Kinetics

The second-order decomposition of NO₂ has a rate constant of 0.255 L mol^-1 s^-1.How much NO₂ decomposes in 4.00 s if the initial concentration of NO₂ (1.00 L volume)is 1.33 mol L^-1?

What is the unit of k in the following rate law? Rate = k[X][Y]²

A reaction with an activation energy of 71.6 kJ mol^-1 has a rate constant of 8.14 L mol^-1 s^-1 at 350 K.At what temperature will the rate constant be one-half?

What is the unit of k in a second-order reaction?

$\mathrm { SO } _ { 2 }$ $\mathrm { Cl } _ { 2 }$ decomposes in the gas phase by the reaction $\mathrm { SO } _ { 2 }$ $\mathrm { Cl } _ { 2 }$ (g)? $\mathrm { SO } _ { 2 }$ (g)+ $\mathrm { Cl } _ { 2 }$ (g) The reaction is first order in $\mathrm { SO } _ { 2 }$ $\mathrm { Cl } _ { 2 }$ and the rate constant is 3.0 × $10 ^ { - 6 }$ $s ^ { - 1 }$ at 600 K.A vessel is charged with 6.4 atm of $\mathrm { SO } _ { 2 } \mathrm { Cl } _ { 2 }$ at 600 K.The partial pressure of $\mathrm { SO } _ { 2 }$ $\mathrm { Cl } _ { 2 }$ at $3.0 \times 10 ^ { 5 } \mathrm {~s}$ is ________ atm.

Which of the following reactions would you predict to have the largest orientation factor?

What is the unit of k in the following rate law? Rate = k[X][Y]

The rate constant for the first-order decomposition of N₂O is 3.40 s^-1.What is the half-life of the decomposition?

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?

Which of the following represents the equation for a second-order half-life?

What is the overall order of the following reaction,given the rate law? 2NO(g)+ H₂(g)→ N₂(g)+ 2H₂O(g)Rate = k[NO]²[H₂]

Given the following balanced equation,determine the rate of reaction with respect to [O₃]. 2O₃(g)? 3O₂(g)

Calculate the temperature if a reaction has a rate constant,k,of 841 s^-1,a frequency factor,A,of 6.0 × 10¹² s^-1,and an activation energy,E_a,of 62 kJ mol^-1.

Calculate the frequency factor,A,for a reaction with a rate constant of 162.3 s^-1 and an activation energy,E_a,of 68 kJ mol^-1 at 298 K.

The combustion of ethylene proceeds by the reaction $\mathrm { C } _ { 2 }$ $\mathrm { H } _ { 4 }$ (g)+ 3 $\mathrm { O } _ { 2 }$ (g)? 2C $\mathrm { O } _ { 2 }$ (g)+ $2 \mathrm { H } _ { 2 }$ O(g) When the rate of disappearance of $\mathrm { O } _ { 2 }$ is 0.74 mol L^-1 $s ^ { - 1 }$ ,the rate of disappearance of $\mathrm { C } _ { 2 }$ $\mathrm { H } _ { 4 }$ is ________ $\mathrm { mol } \mathrm { L } ^ { - 1 } \mathrm {~s} ^ { - 1 }$

What happens to the concentration of reactants and products during a chemical reaction?