Express the rate of the reaction2NO(g)+ Cl2 (g)→ 2NOCI(g)a. in terms of A[NOCI].8 AINOCI]/Atrate =b. in terms of A[Cl2].e A[Cl2]/Atrate =Submit AnswerTry Another Version9 item attempts remaining

Answered: Image /qna-images/answer/0058d164-d24a-4ca7-9434-bbef0bca9d84.jpg

Answered: Express the rate of the reaction…

Express the rate of the reaction 2NO(g)+ Cl2 (g)→ 2NOCI(g) a. in terms of A[NOCI]. rate = e A[NOCI]/At b. in terms of A[Cl2]. rate = A[Cl2]/At

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the rate law of the reaction below: NO (g) + NO (g) -> N202 (g) fast N202(g) + O2(g)-> 2NO2 (g) slow rate = k [NOJ?[02] rate = k [NO]2[02]2 rate k [NO][02] O rate = k [NO][o²j²
The following are initial rate data for: A + 2B - C + 2 D Experiment Initial [A] Initial [B] Initial Rate 1 0.10 0.10 0.300 0.20 0.10 0.600 3 0.10 0.20 1.200 What is the rate law? The rate law is Rate = k[A]?[B]1. The rate law is Rate = k[A]?[B]*. The rate law is Rate = k[A]?[B]°. The rate law is Rate = k[A]°[B]?. The rate law is Rate = k[A]²[B]².
A certain reaction is second order in N, and first order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [H, initial rate of reaction х10 1.26 M 0.560 M 76.0 M/s | M/s 1.26 M 0.272 M | M/s 5.70 M 0.124 M
Consider the reaction:8 H2S(g) + 4 O2(g) ¡ 8 H2O(g) + S8(g)Complete the table.?[H2S]/ ?t ?[O2]/?t ?[H2O], ?t ?[S8], ?t Rate -0.080 M/s
3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. 1 rate = (0.471 M¹S -¹) [N₂05]² Suppose a vessel contains N₂O5 at a concentration of 0.800M. Calculate the concentration of N₂O5 in the vessel 8.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10
1. Which expression does NOT represent the rate of the following reaction? Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) b Δ[Mg] ΔΙ b. Δ[Η,] ΔΙ C. -1 2 ΔHCI] ΔΕ d A[MgCl₂] At
A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4.] initial rate of reaction x10 1.91 M 0.885 M 0.894 M/s olo 0.813 M 0.885 M I|| M/s Ar 0.213 M 7.92 M
10. The data below are for the reaction: 2 NO₂ (g) + F₂ (g) → 2 NO₂F (g) [NO₂] (M) 0.100 0.200 0.200 0.400 0.200 [F₂] (M) 0.100 0.100 0.200 0.400 0.400 Initial rate (M/s) 0.026 0.051 0.103 0.411 see part c a. Write the rate law for this reaction. b. Determine the rate constant for this reaction. Pay attention to units. c. Predict the initial rate of the reaction when [NO₂] = 0.200 M and [F₂] = 0.400 M. d. The mechanism of the reaction is suggested as two steps: NO₂+ F2 → NO₂F + F (fast) NO₂+ F→→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.
A proposed mechanism for the reaction is: - Step 1: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) Step 2: N₂O(g) + H₂(g) → N₂(g) + H₂O(g) What is the rate law? More information is needed to answer this question. Or = K[H₂][NO] Or = K[H₂]²[NO]² Or = K[H₂][NO]² Or=K[H₂]²[NO] (slow) (fast)
Consider the following rate law: Rate = k[B] Which of the following equations could be used to find the concentration of B at some time (t) in the reaction? A) [B] = [B]₀ - kt B) [B] = [B]₀ × e^(-kt) C) 1/[B] = 1/[B]₀ + 2kt D) All of the above