Answer & Solution
Answer: Option C
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2. At T = 300 K, the thermal energy [kBT] in cm-1 is approximately
3. The half-life of a first order reaction varies with temperature according to
4. For a given first order reaction, the reactant reduces to $${\frac{1}{4}^{{\text{th}}}}$$ its initial value in 10 min. The rate constant of the reaction is
5. For the reaction, 2X3 $$ \rightleftharpoons $$ 3X2, the rate of formation of X2 is
6. The half-life time for a reaction at initial concentrations of 0.1 and 0.4 mol-1 are 200 s and 50 s respectively. The order of the reaction is
7. For the reaction shown below,
the value of k1 is 1 × 10-4 s-1. If the reaction starts from X, the ratio of the concentrations of Y and Z at any given time during the course of the reaction is found to be $$\frac{{\left[ {\text{Y}} \right]}}{{\left[ {\text{Z}} \right]}} = \frac{1}{4}.$$ The value of k2 is
the value of k1 is 1 × 10-4 s-1. If the reaction starts from X, the ratio of the concentrations of Y and Z at any given time during the course of the reaction is found to be $$\frac{{\left[ {\text{Y}} \right]}}{{\left[ {\text{Z}} \right]}} = \frac{1}{4}.$$ The value of k2 is
8. Consider an exothermic reaction, $$A\mathop {\mathop \rightleftharpoons \limits_{{k_{ - 1}}} }\limits^{{k_1}} I$$
As the temperature increases
As the temperature increases
9. 1 g of 90Sr gets converted to 0.953 g after 2 yr. The half-life of 90Sr, and the amount of 90Sr remaining after 5 yr are
10. The reaction, 2NO(g) + O2(g) → 2NO2(g) proceeds via the following steps:
NO + NO \[\xrightarrow{{{{\text{K}}_{\text{a}}}}}\] N2O2
N2O2 \[\xrightarrow{{{{\text{K}}_{{\text{a'}}}}}}\] NO + NO
N2O2 + O2 \[\xrightarrow[{\left( {{\text{slow}}} \right)}]{{{{\text{k}}_{\text{b}}}}}\] NO2 + NO2
The rate of this reaction is equal to
NO + NO \[\xrightarrow{{{{\text{K}}_{\text{a}}}}}\] N2O2
N2O2 \[\xrightarrow{{{{\text{K}}_{{\text{a'}}}}}}\] NO + NO
N2O2 + O2 \[\xrightarrow[{\left( {{\text{slow}}} \right)}]{{{{\text{k}}_{\text{b}}}}}\] NO2 + NO2
The rate of this reaction is equal to