Units of rate constant of first and zero order reactions in terms of molarity M unit are respectively
sec–1, M sec–1
sec–1, M
M sec–1, sec–1
M, sec–1
Additional Questions
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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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Rate of a reaction can be expressed by Arrhenius equation as: k = Ae–E/RT In this equation, E represents |
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In a first order reaction, the concentration of the reactant decreases from 0.8 M to 0.4 M in 15 minutes. The time taken for the concentration to change from 0.1 M to 0.025 M is |
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For the reaction, N2 + 3H2 → 2NH3, if $\dfrac{\text{d}NH_3}{\text{d}t}$ = 2 × 10–4 mol L–1 s–1, the value of –$\dfrac{\text{d}H_2}{\text{d}t}$ would be |
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For a reaction $\dfrac{1}{2}$A → 2B, rate of disappearance of 'A' is related to the rate of appearance of 'B' by the expression: |
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For a first order reaction (A) → Product, the concentration of A changes from 0.1 M to 0.025 M in 40 minutes. The rate of reaction when the concentration of A is 0.01 M is: |
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