Chemical Kinetics Tutorials1. Consider the reaction.2HB1(g)H2(g) + Brz(g)a. Express the rate of the reaction in terms of the change in concentration of each of the reactantsand products.b. In the first 25.0 s of this reaction, the concentration of HBr drops from 0.600 M to 0.512 M.Calculate the average rate of the reaction during this time interval.2. For the reaction 2A(g) + B(g) + 3C(g),a. Determine the expression for the rate of the reaction in terms of the change in concentration ofeach of the reactants and products.3. Consider the tabulated data showing the initial rate of a reaction (A » products) at severaldifferent concentrations of A. What is the order of the reaction? Write a rate law for the reactionincluding the value of the rate constant, k.[A] (M)Initial Rate (Ms')0.1000.0530.2000.2100.3000.4734. This reaction is first order in N2O5:N2O5(g) →NO3(g) + NO2(g)The rate constant for the reaction at a certain temperature is 0.053s.a. Calculate the rate of the reaction when [N2O5] = 0.055 M.b. What is the rate of the reaction at the concentration indicated in part a, if the reaction is secondorder? Zero order? (Assume the same numerical value for the rate constant with the appropriateunits.)5. A reaction in which A, B, and C react to form products is firstorder in A, second order in B, and zero order in C.a. Write a rate law for the reaction.b./hat is theorder of thec. By what factor does the reaction rate change if [A] is doubled (and the other reactantconcentrations are held constant)?d. By what factor does the reaction rate change if [B] is doubled (and the other reactantconcentrations are held constant)?e. By what factor does the reaction rate change if [C] is doubled (and the other reactantconcentrations are held constant)?

We are given with a reaction 2HBr ---> H2+Br2 And are asked to give the formula the rate of…

Chemical Kinetics Tutorials 1. Consider the reaction. 2HB1(g) H2(g) + Brz(g) a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. b. In the first 25.0 s of this reaction, the concentration of HBr drops from 0.600 M to 0.512 M. Calculate the average rate of the reaction during this time interval. 2. For the reaction 2A (g) + B(g) 3C(e)

Chemical Kinetics Tutorials 1. Consider the reaction. 2HB1(g) H2(g) + Brz(g) a. Express the rate of the reaction in terms of the change in concentration of each of the reactants and products. b. In the first 25.0 s of this reaction, the concentration of HBr drops from 0.600 M to 0.512 M. Calculate the average rate of the reaction during this time interval. 2. For the reaction 2A (g) + B(g) 3C(e)

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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(Can I get the answer in not more than 45 mins please? or asap. Thank you!)
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Consider the following balanced chemical equation: H₂O2 (aq) + 31 (aq) + 2 H* (aq) → 13¯ (aq) + 2 H₂O (1) In the first 49.9 seconds of the reaction, the concentration of 13 increased from 0.692 M to 0.93 M. What is the average reaction rate over this time interval (in mol L-¹ s-¹)? Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:
2. What is the rate law for the theoretical reaction 2 A + B C + 2 D? a. rate = K[A]² [B] b. It is impossible to determine from this information. c. rate= K[C][D]² d. rate = k[A][B]
The reaction A+B -->C has the following rate law. Rate =k [A] [B]2 If the concentration of A is held constant and B is tripled (x3), by what factor will the rate change? Select one: a. It won’t change b. x9 c. x3 d. x 1/3 e. x6
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Answer all questions in this section. 1. (a) H2S(aq) + Cl2(g) – S(s) + 2HCI(aq) i. Given that, when the concentration of H2S is doubled, rate also double while double the concentration Cl2 will cause the rate of reaction increase 4 times. Write the rate law of the reaction. ii. The overall reaction order ii. The rate of reaction at 300K if the rate constant is 2.8 x 10²M²s' and the concentration of H2S and Cl2 are 2.7×10²M and 7.0x10² M respectively.
2. One method for the destruction of ozone in the upper atmosphere is: O,+ NO → NO, + O,(slow) NO, + 0→ NO + O, (fast) overall rxn: 0, + 0 → 20, a. Which species is an intermediate? b. Which species is a catalyst? c. Which is the rate-determining step (rds)? d. Write the rate law for the reaction?
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Rate law: 3A(g) + B(g) + 2C(g) → D(g) + 2E(g) Rate of formation of D= k [A] [B]2 Doubling the concentration of B increases the rate of reaction by a factor of? a. 9 b. 2 c. 3 d. 4