Consider the reaction, 2A + B → Products. When concentration of B alone was doubled, the half–life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:
The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of reaction with respect to reactant B is |
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For a reaction A + B → C + D if the concentration of A is doubled without altering the concentration of B, the rate gets doubled. If the concentration of B is increased by nine times without altering the concentration of A, the rate gets tripled. The order of the reaction is |
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In respect of the equation K = A–Ea / RT |
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The concentration of R in the reaction R → P was measured as a function of time and the following data is obtained
The order of the reaction is |
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A reaction involving two different reactants can never be |
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Which of the following statements for order of reaction is not correct? |
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The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol–1. The ratio of rate constant to the Arrhenius factor is |
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The following mechanism has been proposed for the reaction of NO and Br2 to form NOBr NO(g) + Br2(g) ⇌ NOBr2(g) NOBr2(g) + NO(g) → 2NOBr(g) If the second step is rate determining step, the order of the reaction with respect to NO(g) is |
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The following data were obtained during the first order decomposition of 2A(g) → B(g) + C(s) at a constant volume and at a particular temperature.
The rate constant in min–1 is |
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Consider an endothermic reaction, X → Y with activation energies Eb and Ef respectively for the backward and forward reactions, respectively. In general, |
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