The rate law of a particular reaction is found to be, rate = k[A]²[B]. Which of the following statements is %3D FALSE? The actual value of k will depend on the temperature The actual value of k will depend on the concentrations of A and B The units of k could be (L²/mol² s) Tripling the concentration of A will result in a nine-fold increase in the rate The reaction is third order overall.

The rate law of a particular reaction is found to be, rate = k[A]²[B]. Which of the following statements is %3D FALSE? The actual value of k will depend on the temperature The actual value of k will depend on the concentrations of A and B The units of k could be (L²/mol² s) Tripling the concentration of A will result in a nine-fold increase in the rate The reaction is third order overall.

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

At a certain temperature the rate of this reaction is second order in HI with a rate constant of 0.22M¹s¹: 2 HI(g) → H₂(g) + 1₂ (8) Suppose a vessel contains HI at a concentration of 0.910M. Calculate how long it takes for the concentration of HI to decrease to 0.064 M. You may assume no other reaction is important. Round your answer to 2 significant digits. 0.9 X 圖图

A student ran several experiments for this reaction: 5 CH3COOH(aq) + 8 MnO4 (aq) + 24 H*(aq) → 8 Mn2 (aq) + 10 CO₂(g) + 22 H₂O(l) One of the experiments gave this data: Experiment # [CH3COOH] (M) 0.269 3 [MnO4] (M) 0.395 The student determined the rate law to be: ratek [CH3COOH)² [MnO4)² [H*] Calculate k for this reaction. I [H] (M) 0.245 initial rate (M/s) 0.228
Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S
Consider the initial-rate data at a certain temperature in the table for the reaction described by 2 NO₂(g) + O₂(g) → N₂O5 (g) + O₂(g) Determine the value and units of the rate constant, k. k = X10 TOOLS [NO2], (M) [03]o (M) 0.650 0.800 1.10 0.800 1.76 1.40 Units: Initial rate (M/s) 3.12 x 104 5.28 x 104 14.78 x 104
The rate of a certain reaction is given by the following rate law: rate =k N, O, Use this information to answer the questions below. olo What is the reaction order in N,? |x10 18 Ar What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of reaction is 0.780 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103M/s when [N2] = 1.1 M and [03] = 1.1 M. Calculate the value of - 3 -1 k = |M •S the rate constant. Round your answer to 2 significant digits.
Initial rate: 1.6 •10^-7mol/L•s K=6.4 •10^-9L/mol•s Rate law: k[HI]^2 Can you please show me the steps.
Consider this reaction: 2HI (g) → H, (g) +I, (g) At a certain temperature it obeys this rate law. rate =(0,465 s)[HI Suppose a vessel contains HI at a concentration of 0.540M. Calculate the concentration of HI in the vessel 2.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (8.98 × 10-4 ')[c,os] -1 S Suppose a vessel contains Cl₂05 at a concentration of 1.40M. Calculate the concentration of Cl₂O5 in the vessel 690. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
Consider this reaction: 2H1 (g) → H₂(g) +1₂(e) At a certain temperature it obeys this rate law. rate = (0.345-¹) [HI] Suppose a vessel contains HI at a concentration of 0.730M. Calculate how long it takes for the concentration of HI to decrease by 86.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0. 08
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
The rate of a certain reaction is given by the following rate law: rate=k|N, || H2 K[N][H° Use this information to answer the questions below. What is the reaction order in N,? 1 х10 What is the reaction order in H2? ? 2 What is overall reaction order? 3 At a certain concentration of N, and H2, the initial rate of M reaction is 5.0 x 103 M / s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round S your answer to 2 significant digits. The rate of the reaction is measured to be 0.640 M/ s when [N2] - 2 • S 1.8 M and [H2] 1.4 M. Calculate the value of the rate - 1 k = |M constant. Round your answer to 2 significant digits.