(a)
Interpretation:
The order with respect to each reactant and the overall order of the reaction have to be determined.
Concept Introduction:
The rate of the reaction is referred to the change in the molar concentration in the distinct interval of time. According to the rate law, the rate of the reaction is directly proportional to the initial concentration of the reactant of the reaction.
(b)
Interpretation:
The expression for the rate law has to be determined.
Concept Introduction:
Same as part (a).
(c)
Interpretation:
The rate constant for the given reaction has to be determined.
Concept Introduction:
Same as part (a).
(d)
Interpretation:
The
Concept Introduction:
Same as part (a).
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Chemical Principles: The Quest for Insight
- Consider the reaction A + B ¡ C + D. Is each of the following statements true or false? (a) The rate law for the reaction must be Rate = k3A43B4. (b) If the reaction is an elementary reaction, the rate law is second order. (c) If the reaction is an elementary reaction, the rate law of the reverse reaction is first order. (d) The activation energy for the reverse reaction must be greater than that for the forward reaction.arrow_forwardThe radioactive isotope 28Mg has a half-life of 20.9 hours. (a) What is the rate constant for this first-order reaction? (b) What fraction of the isotope remains after 24 hours? Assume 3 significant figures in your calculations.arrow_forward(a) For a reaction, A + B > Product, the rate law is given by,Rate = k [A]1 [B]2 . What is the order of reaction?(b) Write the unit of rate constat ‘k’ for the first order reaction.arrow_forward
- The decomposition of XY is second order in XY and has a rate constant of 7.41 × 10−3 L·mol−1·s−1 at a certain temperature, the half-life for this reaction at an initial concentration of 0.101 mol·L−1 1336. A) If the initial concentration of XY is 0.225 mol·L−1, how long will it take for the concentration to decrease to 6.95 × 10−2 mol·L−1 ?, B) If the initial concentration of XY is 0.080 mol·L−1, what is the concentration of XY after 75 s ?arrow_forwardConsider the following reaction:2 NO(g) + 2 H2(g)--->N2(g) + 2 H2O(g)(a) The rate law for this reaction is first order in H2 andsecond order in NO. Write the rate law. (b) If the rateconstant for this reaction at 1000 K is 6.0 x 104 M-2 s-1,what is the reaction rate when [NO] = 0.035 M and[H2] = 0.015 M? (c) What is the reaction rate at 1000 Kwhen the concentration of NO is increased to 0.10 M,while the concentration of H2 is 0.010 M? (d) What is thereaction rate at 1000 K if [NO] is decreased to 0.010 M and[H2] is increased to 0.030 M?arrow_forwardThe following kinetic data are collected for the initial rates of a reaction 2 X + Z→ products: Experiment [X ]o(M) [Z]o(M) Rate (M/s) 0.25 0.25 4.0 x 10! 0.50 0.50 3.2 x 102 0.50 0.75 7.2 x 102 (a) What is the rate law for this reaction? (b) What is the value of the rate constant with proper units? (c) What is the reaction rate when the initial concentration of X is 0.75 M and that of Z is 1.25 M? 2. 3.arrow_forward
- Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/sarrow_forward(a) For a reaction A + B —> P, the rate is given by Rate = k[A]2 [B](i) How is the rate of reaction affected if the concentration of A is doubled?(ii) What is the overall order of reaction if B is present in large excess?(b) A first order reaction takes 23.1 minutes for 50% completion. Calculate the time required for 75% completion of this reaction.(Given: log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021)arrow_forwardThe following data were measured for the reaction of nitricoxide with hydrogen:2 NO(g) + 2 H2(g)------>N2(g) + 2 H2O(g)(a) Determine the rate law for this reaction.(b) Calculate the rate constant.(c) Calculate the rate when [NO] = 0.050 M and[H2] = 0.150 M.arrow_forward
- 6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO2 (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?arrow_forwardThe reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?arrow_forward1. Which of the following statements is incorrect? (A) As the chemical reaction proceeds, the rate of reaction increases. (B) The reaction rate almost gets doubled for 10°C rise in temperature. (C) For a first order chemical reaction, the rate constant has unit of time-1. (D) Chemical kinetics can predict the rate of a chemical reaction. 2. In a chemical reaction, represented by A → P, it is observed that the rate of reaction increases by a factor of 4 on doubling the concentration of the reactant. The rate of reaction increases by a factor of 9 on trebling the concentration of the reactant. Then the rate of the reaction is proportional to (A) CA (B) CA2 (C) CA3 (D) CA4 3. An elementary reaction has the stoichiometric equation A + 2B = P. What is the order of reaction (A) 0 (B) 1 (C) 2 (D) 3 4. It states that the rate of a chemical reaction is directly proportional to the product of the activities or concentrations of the reactants. (A) Law of mass action…arrow_forward
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