(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 relationship between the rate of a reaction and its activation energy.arrow_forward. Account for the increase in reaction rate brought about by a catalyst.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 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_forwardWhen heated, cyclopropane is converted to propene. Rate constants for this reaction at 470. °C and 510. °C are ki = 1.10 x 104 s and k2 = 1.02 x 10s, respectively. Determine the activation energy, Ea, from these data. The gas constant R is 8.3145 x 10 3 kJ/mol · K. E = kJ/molarrow_forwardConsider the following reaction: (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? Rate = k [HBr(g)] [O₂(g)] O Rate = k [HBr(g)]² [O₂(g)] O Rate = k [HBr(g)] [O₂(g)]² O Rate = k [HBr(g)]² [0₂(g)]² O Rate = k [HBr(g)] [O₂(g)]³ O Rate = k [HBr(g)]4 [0₂(g)] (b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.00876 M? Rate = 4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M? M/Sarrow_forward
- The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E=22.0 kJ/mol. If the rate constant of this reaction is 1.1 x 108 M¹s¹ at 309.0 °C, what will the rate constant be at 277.0 °C? Round your answer to 2 significant digits. k = M¹ s ? dlarrow_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_forwardGiven the following values of the enthalpy (DH) and activation energy (Ea) of four different reactions, identify an exothermic reaction that would exhibit the fastest rate at 298 K. (Assume that all reactants have the same initial concentration and the same Arrhenius frequency factor A in k = Ae-Ea/RT). (A) DH = +45 kJ/mol; Ea = 75 kJ/mol; (B) DH = +35 kJ/mol; Ea = 65 kJ/mol; (C) DH = -35 kJ/mol; Ea = 75 kJ/mol; (D) DH = -45 kJ/mol; Ea = 65 kJ/mol;arrow_forward
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