(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
- (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_forwardConsider 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 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_forward
- The 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_forwardConsider 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_forward
- Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this reaction is second order in NO(g) and first order in H2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 79200, what is the reaction rate when [NO(g)] = 0.0852 M and [H2(g)] = 0.137 M?Rate =____ M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.170 M while the concentration of H2(g) is 0.137 M?Rate = ____ M/sarrow_forward6. 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 initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, karrow_forward
- The 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_forwardThe reaction 2 NO(g) + Cl2(g) → 2 NOCl has the following rate law: Rate = k[NO]2 [Cl2]. The initial speed of the reaction was found to be 5.72×10‒6 M/s when the reaction was carried out at 25 °C with initial concentrations of 0.500 M NO and 0.250 M Cl2. What is the value of k?(a) 1.83×10‒4(b) 1.09×104(c) 9.15×10‒5(d) 5.72×10‒6arrow_forwardConsider the following reaction: O2(g) + 2 NO(g) 2 NO2(g)(a) The rate law for this reaction is first order in O2(g) and second order in NO(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 7840, what is the reaction rate when [O2(g)] = 0.0162 M and [NO(g)] = 0.0299 M?Rate = _____ M/s.(c) What is the reaction rate when the concentration of O2(g) is doubled, to 0.0324 M while the concentration of NO(g) is 0.0299 M?Rate = _____ M/sarrow_forward
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