For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H2S(g) + O2l) → 2S(s) + 2H2O() Multiple Choice The reaction is second-order overall. The rate law is: rate - KH257 (02). The reaction is third-order overall. The rate law cannot be determined from the information given. The rate law is: rate KH2S][O2)

For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H2S(g) + O2l) → 2S(s) + 2H2O() Multiple Choice The reaction is second-order overall. The rate law is: rate - KH257 (02). The reaction is third-order overall. The rate law cannot be determined from the information given. The rate law is: rate KH2S][O2)

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...

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3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096
The reaction in aqueous acidic solution occurs as shown by the balanced chemical equation below: H2O2(aq) + 3 I (aq) + 2 H* (aq) 13 (aq) + 2 H20(I) In the first 40.0 seconds of the reaction, the concentration of I' changes from 1.000 M to 0.868 M. Use the information to determine the average rate of the reaction within the first 40.0 seconds of the reaction. O 3.20x103 M/s O 1.10x10-3 M/s O 4.40x10-3 M/s O 2.20x10-3 M/s
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
Consider the elementary reaction of nitric oxide (NO) and diatomic fluorine (F,) to form nitrosyl fluoride (NOF) and monatomic fluorine (F). NO(g) + F,(g) → NOF(g) + F(g) Write the rate law for this elementary reaction. (Rate expressions take the general form: rate = k. [A]a . [B]Þ.) chemPad Help XX"| →e- Greek
Consider the following reaction: 2 H2O2(aq) + I–(aq) -> 2 H2O(l) + O2(g) + I–(aq) Suppose we were able to measure the amount of oxygen gas formed in units of moles/L, and the rate of formation of oxygen was found to be 0.0125 M/s. Using the rate law for this reaction and the units associated with each variable, show what the derived units for the rate law constant would be.
for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction
Rate laws are determined experimentally by varying the concentrations of the reactants and observing the effect on the initial rate. Concentration and rate data are provided in the table below for the reaction shown. 2NO(g) + Cl2(g) -> 2NOCl(g) Experiment [NO](M) [Cl2] (M) Initial Rate (M/s) 1 0.20 0.10 0.63 2 0.20 0.30 5.70 3 0.80 0.10 2.58 4 0.40 0.20 ? Predict the rate for experiment 4, given the other concentration/rate data provided. _____M/s
A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]
Consider the experimental data collected for the following chemical reaction: 2H2(g) + 2NO(g) → N2(g) + 2H2O(g) Trial Initial [H2] (mol/L) Initial [NO] (mol/L) Rate of Reaction (mol/L∙s) 1 0.031 0.0025 2.0 x 10-3 2 0.062 0.0025 4.0 x 10-3 3 0.031 0.0050 8.0 x 10-3 4 0.062 0.0050 1.6 x 10-2 Which action will have more effect on the rate of this reaction; changing the concentration of H2(g) or that of NO(g)? Explain your reasoning by considering the orders of reactants and writing the corresponding rate law equation.
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.
A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻ because it is first order for I - . After you find the reaction order for S2O82⁻ you need to calculate k. S2O82⁻ (aq) + 3 I⁻ (aq) → 2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 ) 0.30 0.42 4.54 0.44 0.42 6.65 Rate = 120 M-2s-1 [S2O82⁻]2[I⁻] Rate = 195 M-3s-1 [S2O82⁻]2[I⁻] Rate = 86 M-2s-1 [S2O82⁻][I⁻] Rate = 23 M-1/2s-1 [S2O82⁻][I⁻] Rate = 36 M-1s-1 [S2O82⁻][I⁻]
Consider this reaction: 2C1,0, g) → 2C1, (6) + 50, (g) At a certain temperature it obeys this rate law. rate = (0.36 Ms)[C1,0,1 %3D Suppose a vessel contains Cl,0, at a concentration of 0.630 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 5.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.