The reaction 2 NO(g) + O 2 (g) → 2 NO 2 (g) is second order in NO and first order in O 2 . When [NO] = 0.040 M, and [O 2 ] = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10 -5 M/s. (b) What is the value of the rate constant?

everyone to wear direction below. And the reaction is second order in nitric oxide impressed order and chlorine gas. And the rate of disappearance is 3.44 cents to four m/s When the concentration of magic oxide and chlorine gas are $2.5 and tube boiler. Or as conflict the value of the rate constant. We know that the right long equation is rape Equals rate constant. Construction of eight. The power of X and X. Is the order with respect to a concentration of B. The power of why and why is the order with respect to be over this our rate if it's okay. Construction of magic outside the power of X. Construction of chlorine gas, the power of why so far right. We're gonna have the right concept, concentrate on the match outside to the second power because we have second order in natural oxide construction of chlorine gas for the first power. Our first order and flowing gas. We know that our rate. It was 3.44 Have 10 to the four mile per second in the concentrations oxide in flooring gas or 2.5 Muller and to Mueller. If we plug in our values, we're gonna get 3.44 sensitive for per second. He goes to the right constant, Times 2.5 More where times to Mahler You get 3.44 times 10 to the four mile per second. It was the right constant. That's 12.5 more cute for the right constant. We get 2.75 since the third bullet to the negative. Two power from second to mega one power. Thanks for watching my video. And I hope it was helpful.

Ch.14 - Chemical Kinetics

All textbooks

Brown 15th Edition

Ch.14 - Chemical Kinetics

Problem 91b

Chapter 14, Problem 91b

The reaction 2 NO(g) + O₂(g) → 2 NO₂ (g) is second order in NO and first order in O₂. When [NO] = 0.040 M, and [O₂] = 0.035 M, the observed rate of disappearance of NO is 9.3⨉10^-5 M/s. (b) What is the value of the rate constant?

Verified step by step guidance

Identify the rate law for the reaction. Since the reaction is second order in NO and first order in O_2, the rate law is: rate = k[NO]^2[O_2].

Substitute the given concentrations and the rate of disappearance into the rate law equation. You have: 9.3 \times 10^{-5} \text{ M/s} = k (0.040 \text{ M})^2 (0.035 \text{ M}).

Solve the equation for the rate constant k. Rearrange the equation to isolate k: k = \frac{9.3 \times 10^{-5} \text{ M/s}}{(0.040 \text{ M})^2 (0.035 \text{ M})}.

Calculate the value of k using the rearranged equation. Ensure that you perform the arithmetic operations correctly to find the numerical value of k.

Remember to include the correct units for the rate constant k. Since the reaction is third order overall (second order in NO and first order in O_2), the units for k will be M^{-2} s^{-1}.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Rate Law

The rate law expresses the relationship between the rate of a chemical reaction and the concentration of its reactants. For the given reaction, the rate law can be written as Rate = k[NO]^2[O2]^1, where k is the rate constant. Understanding the rate law is essential for determining how changes in concentration affect the reaction rate.

Order of Reaction

The order of a reaction refers to the power to which the concentration of a reactant is raised in the rate law. In this case, the reaction is second order with respect to NO and first order with respect to O2. The overall order of the reaction is the sum of the individual orders, which helps in calculating the rate constant and understanding the kinetics of the reaction.

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that is specific to a given reaction at a certain temperature. It reflects the speed of the reaction and can be determined using the observed rate and concentrations of the reactants. Calculating k is crucial for predicting how the reaction will behave under different conditions.