Question

Need help with part B and C

<Assignment 15 Chap 14: Determining Rate Laws Problem 14.30 - Enhanced - with Feedback ® 3014 ~ M Review | Constants Periodic Table Consider the following reaction: 2NO(g) + 2H2(g) →N2(g) + 2H2O(g). You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. If the rate constant for this reaction at 1000 K is 6.0 x 104 M-s-7, what is the reaction rate when (NO) = 2.80x10-2 M and H2] = 1.90x10-2 M? Express your answer using two significant figures. O ALQ O 2 ? rate = 1.8 M/S Submit Previous Answers Request Answer X Incorrect; Try Again; 8 attempts remaining Part C What is the reaction rate at 1000 K when the concentration of NO is increased to 0.11 M while the concentration of H, is 1.90x10-2 M? Express your answer using two sianificant figures

Answer 1

Cat B Rate = K[A] [B7h k- Rate constant mins rate (MS-1)=k [NO] ² [H₂] = 6 x 10+4 M-2812.0 x 10-2MTc.gx10-2M] = 0. 894 Ms-1 Part ( [no]=0.11M Rate (MS-1) = 68 104 M-2g+Coulm] [1.98 10-2 M] = .8 13.794 Ms"! Note The units of rate constant tell that the reaction is third serden. But we dont know if the reaction is third order in one reactant or first in one and second-order in other since the second question involves changing concentration! of No, we assume that the reaction is second order with respect to No