Question 11.8: Some of the damage to the ozone layer of the upper atmospher...

Physical Chemistry [EXP-34184]

Some of the damage to the ozone layer of the upper atmosphere might involve the reaction

NO+O_{3} → NO_{2}+O_{2}

The reaction is first order in each reactant and the rate constant is equal to $1.3×10^{6} L mol^{−1} s^{−1}$ at 298 K. If the initial concentrations of NO and $O_{3}$ are both equal to $1.00×10^{−6} mol L^{−1}$ , find the concentrations of NO and $O_{3}$ at time t=2.00 s.

The "Step-by-Step Explanation" refers to a detailed and sequential breakdown of the solution or reasoning behind the answer. This comprehensive explanation walks through each step of the answer, offering you clarity and understanding.
Our explanations are based on the best information we have, but they may not always be right or fit every situation.

The Blue Check Mark means that this solution has been answered and checked by an expert. This guarantees that the final answer is accurate.
Learn more on how we answer questions.

This Question has been Answered.

Already have an account?

Login

Related Answered Questions

For a hypothetical isomerization that is first order in both directions with kf=17.7 min^−1 and kr=32.2 min^−1, find the equilibrium composition if the initial concentration of A is equal to 0.175 mol L^−1 and the initial concentration of B is equal to zero. Find the half-life and the relaxation

Verified Answer:

K=\frac{k_{f}}{k_{r}} =\frac{17.7 min^{−1}}...

At 25°C, the forward rate constant of Eq. (11.7-10) is equal to 1.4×10^11 Lmol^−1 s^−1. At this temperature, the dissociation equilibrium constant Kw equals 1.008×10^−14 mol^2 L^−2. a. Using Eq. (11.5-3), find the value of k′1. b. For pure water, find the relaxation time if a T-jump experiment has

Verified Answer:

a. We convert

K_{w}

, for which the ...

The following data were taken at 298K for the gas-phase reaction Find the order with respect to each reactant and find the rate constant.

Verified Answer:

In this case we proceed algebraically since there ...

For the gas-phase reaction at 300°C: C2F4 → 1/2 cyclo-C4F8 the following data on the concentration of C2F4 were taken. Determine the order of the reaction and the rate constant at this temperature. Assume that the reverse reaction is negligible.

Verified Answer:

This example can be solved by inspection. Each con...

Following are data for the decomposition of ethyl chloride, C2H5Cl, at 500°C. Find the order of the reaction and the rate constant at this temperature.

Verified Answer:

A linear least-squares fit of

\ln(r_{initia...

Assume that for the reaction NO+O3→NO2+O2 [NO]0=1.00×10^−6 mol L^−1 and [O3]0=5.00×10^−7 mol L^−1. Find the concentration of O3 after 3.50 s.

Verified Answer:

Let

O_{3}

be denoted by A and NO be...

A hypothetical zero-order reaction has a rate constant equal to 0.0150 mol L^−1 s^−1 at a certain temperature. If the initial concentration of the single reactant is 1.000 mol L^−1, find the concentration after a reaction time of 5.00 s at this temperature.

Verified Answer:

[A]_{t}=[A]_{0} − k_{f} t=1.000 mol L^{−1} ...

The gas-phase reaction N2O5 → 2NO2+1/2O2 is found to be first order. The rate constant at 337.6K is equal to 5.12×10^−3 s^−1.^a If the partial pressure of N2O5 is 0.500 atm at time t=0, find the partial pressure of N2O5 at t=60.0 s, neglecting any reverse reaction and assuming that the system is

Verified Answer:

Assuming the gas to be ideal, the partial pressure...

The gas-phase reaction NO3 → NO2+1/2 O2 obeys second-order kinetics. At a temperature of 20°C and an initial concentration of NO3 equal to 0.0500 mol L^−1 , the concentration after 60.0 minutes is equal to 0.0358 mol L^−1. Assuming the reverse reaction to be negligible, find the value of the

Verified Answer:

k_{f}=\frac{1}{t}\Bigl(\frac{1}{[NO_{3}]_{t...

Find the half-life of the reaction of the previous example with the given initial concentration.

Verified Answer:

t_{1/2}=\frac{1}{k[NO_{3}]_{0}} =\frac{1}{(...