(a)
Interpretation:
The activation energy for the isomerization reaction of cyclopropane to propene has to be calculated.
Concept Introduction:
The temperature dependence of rate constant can be explained through Arrhenius equation.
Where
The logarithmic form of Arrhenius is given below.
Where,
(b)
Interpretation:
The time taken for the concentration drop from
Concept Introduction:
The temperature dependence of rate constant can be explained through Arrhenius equation.
Where
The logarithmic form of Arrhenius is given below.
Where,
The integrated rate law for a first order reaction is given below.
Where
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Chapter 11 Solutions
Chemistry: The Molecular Science
- . Account for the increase in reaction rate brought about by a catalyst.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_forwardHydrogen peroxide decomposes spontaneously to yield water and oxygen gas according to the reaction equation 2 H2O2(aq)⟶2 H2O(l)+O2(g) The activation energy for this reaction is 75 kJ⋅mol−1. In the presence of a metal catalyst, the activation energy is lowered to 49 kJ⋅mol−1. At what temperature would the non‑catalyzed reaction need to be run to have a rate equal to that of the metal‑catalyzed reaction at 25 ∘C?arrow_forward
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- 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: 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 9.70e+04, what is the reaction rate when [NO(g)] = 0.0560 M and [H2(g)] = 0.119 M?Rate = M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.112 M while the concentration of H2(g) is 0.119 M?Rate = M/sarrow_forwardConsider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? O Rate = k [NO₂(g)] [03(9)] Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(9)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(9)] (b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [O3(9)] = 1.42 M? Rate = 2 NO₂(g) + 03(g) → N₂05(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M? M/sarrow_forward
- For the reversible, one-step reaction, A + A k₁ K = k-1 B + C the rate constant for the forward reaction, k₁, is 265 L·mol¯¹·min¯¹ and the rate constant for the reverse reaction, k₁, is 385 L·mol¯¹·min¯¹ at a given temperature. The activation energy for the forward reaction is 42.9 kJ.mol-¹, whereas the activation energy for the reverse reaction is 23.0 kJ.mol-¹. Determine the equilibrium constant, K, of this reaction.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_forwardA particular second-order reaction has a rate constant of 2.4 x 10–6 M–1 s–1 at 575 K and 6.0 x 10–5 M–1 s–1 at 630 K. (a) Calculate the activation energy of the reaction. (b) What is the value of the rate constant at 25°C?arrow_forward
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