The activation energy for a reaction at the temperature T K was found to be 2.303 RT J mol–1. The ratio of the rate constant to Arrhenius factor is ______.
10–1
10–2
2 × 10–3
2 × 10–2
Additional Questions
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In a zero–order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become |
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The bromination of acetone that occurs in acid solution is represented by the equation CH3COCH3(aq) + Br2(aq) → CH3COCH2Br(aq) + H+(aq) + Br–(aq) These kinetic data were obtained from given reaction concentrations.
Initial Rate, disappearance of Br2, ms–1 (a)5.7 × 10–5 (b)5.7 × 10–5 (c)1.2 × 10–4 (d)3.1 × 10–4 Based on these data, the rate of reaction is |
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Which of these does not influence the rate of reaction? |
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The rate constants k1 and k2 for two different reactions are 1016 × e–2000/T and 1015 × e–1000/T, respectively. The temperature at which k1 = k2 is |
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Units of rate constant of first and zero order reactions in terms of molarity M unit are respectively |
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If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately |
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In a first order reaction A → B, if k is rate constant and initial concentration of the reactant A is 0.5 M, then the half–life is |
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Consider the reaction: N2(g) + 3H2(g) → 2NH3(g) The equality relationship between $\dfrac{\text{d}[NH_3]}{\text{d}t}$ and $\dfrac{\text{d}[H_2]}{\text{d}t}$ is |
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For the reaction: 2A + B → 3C + D, which of the following does not express the reaction rate? |
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The energies of activation for forward and reverse reactions for A2 + B2 ⇌ 2AB are 180 kJ mol–1 and 200 kJ mol–1 respectively. The presence of a catalyst lowers the activation energy of both (forward and reverse) reactions by 100 kJ mol–1. The enthalpy change of the reaction (A2 + B2 → 2AB) in the presence of catalyst will be (in kJ mol–1): |
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