Please use the values in the resources listed below instead of the textbook values. Tripling the concentration of a reactant increases the rate of a reaction nine times. With this knowledge, answer the following questions. (a) What is the order of the reaction with respect to that reactant? zero first second third (b) Increasing the concentration of a reactant by a factor of four increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant? zero first second third

Please use the values in the resources listed below instead of the textbook values. Tripling the concentration of a reactant increases the rate of a reaction nine times. With this knowledge, answer the following questions. (a) What is the order of the reaction with respect to that reactant? zero first second third (b) Increasing the concentration of a reactant by a factor of four increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant? zero first second third

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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Doubling the concentration of a reactant increases the rate of a reaction two times. With this knowledge, answer the following questions. (a) What is the order of the reaction with respect to that reactant? (b) Increasing the concentration of a reactant by a factor of four increases the rate of a reaction sixteen times. What is the order of the reaction with respect to that reactant?
Part A) The rate constant for a certain reaction is k = 8.80×10−3 s−1. If the initial reactant concentration was 0.550 M, what will the concentration be after 18.0 minutes? Express your answer with the appropriate units. Part B) A zero-order reaction has a constant rate of 3.80×10−4 M/s. If after 45.0 seconds the concentration has dropped to 4.50×10−2 M, what was the initial concentration? Express your answer with the appropriate units.
The gas phase reaction, Cl(g) + HBr(g) –→ HCI(g) + Br(g) has an overall enthalpy change of -66 kJ. The activation energy for the reaction is 7 kJ. What is the activation energy for the reverse reaction? (Tip: Draw an energy profile diagram of the forward reaction to help you visualize it.) Report your answer in standard notation to the ones place and do not include units (kJ).
The rate of a certain reaction is given by the following rate law: rate = Use this information to answer the questions below. What is the reaction order in N2? 3 What is the reaction order in O3? 1 What is overall reaction order? At a certain concentration of N2 and Oz, the initial rate of reaction is 7.0 x 105 M / s, What would the initial rate of the reaction be if the concentration of N, were doubled? Round your answer to 2 significant digits. The rate of the reaction is measured to be 0,.700M/s when [N2] = 0.91 M and [03] = 0.74 M. Calculate the value of the k = rate constant. Round your answer to 2 significant digits. Continue Submit Assignment O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use I Privacy Accessibility 回国
Consider the reaction: 4 A + 7 B → 4 C + 6 D At a certain instant, the initial rate of disappearance of the reactant B is X. a) What is the initial rate of the appearance of product D at the same instant? [ Select ] b) The average rate of appearance of product D in the reaction is found to be 4.23 x 102 M over a certain interval of time. What is the rate of disappearance of reactant B during this interval? [ Select ] c) Assume that the rate law of the reaction is given by Rate = k{B}. The reaction takes 36 s to consume 25% of reactant B. Calculate the percentage remaining of reactant B after another 80 s in the same reaction. [ Select ]
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Consider the data showing the initial rate for the reaction CH3CI(g) + 3 Cl2(g)→CCI4(g) + 3 HCI(g) at several different concentrations. What is the overall order of the reaction? Write a rate law for the reaction, including the value of the rate constant, k. [CH3CI] (M) (Cl2] (M) Initial Rate (Ms) 0.050 0.050 0.014 0.100 0.050 0.029 0.100 0.100 0.041 0.200 0.200 0.115
The rate of a certain reaction is given by the following rate law: rate =k Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N2 and H2, the initial rate of M reaction is 8.0 x 104 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 0.820 M / s when [N2] = 0.66 M and [H2] = 1.5 M. Calculate the value of the k = M -2 - 1 S. rate constant. Round your answer to 2 significant digits.
The rate of a certain reaction is given by the following rate law: e=k[H₂] [NH₂] Use this information to answer the questions below. rate = What is the reaction order in H₂? What is the reaction order in NH3? What is overall reaction order? At a certain concentration of H₂ and NH3, the initial rate of reaction is 5.0 x 104 M/s. What would the initial rate of the reaction be if the concentration of H₂ were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 29.0 M / s when [H₂] = 0.99 M and [NH3] = 1.7 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. k = M 0 0 0 M 04/1 2 - 1 'S x10 X
a) What is the rate constant for this reaction? b) If the volume of the reaction container is decreased by a factor of 2 (the volume is cut in half), will the reaction rate be faster or slower? By what factor will the rate of the reaction change?