A reaction was found to be second order with respect to concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will
The half life period of a first order chemical reaction is 6.93 minutes. The time required for the completion of 99% of the chemical reaction will be (log 2 = 0.301) |
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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 ______. |
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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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