Medium
Rate of reaction for $2X + Y \rightarrow 3W + Z$ is $1.2 \times 10^{-4} \ mol \ dm^{-3} \ sec^{-1}$ when $[X] = [Y] = 0.6 \ mol \ dm^{-3}$. Calculate the value of the rate constant if the reaction is first order in $X$ and zero order in $Y$.
- A$2 \times 10^{-4} \ sec^{-1}$
- B$6 \times 10^{-3} \ mol \ dm^{-3} \ sec^{-1}$
- C$4 \times 10^{-4} \ sec^{-1}$
- D$1.8 \times 10^{-3} \ mol \ dm^{-3} \ sec^{-1}$
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Similar Questions
The rate for the reaction $2 A + B \rightarrow \text{product}$ is $6 \times 10^{-4} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is first order in $A$ and zeroth order in $B$,given $[A] = [B] = 0.3 \ M$.
Write the unit of the rate constant for the following reactions:
$1.$ $\frac{1}{2}$ order
$2.$ $\frac{3}{2}$ order
$1.$ $\frac{1}{2}$ order
$2.$ $\frac{3}{2}$ order
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View SolutionWhich among the following is a false statement?
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View SolutionThe mechanism of the reaction,$2NO_{(g)} + 2H_{2(g)} \to N_{2(g)} + 2H_2O_{(g)}$ is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is:
Step $1$: $2NO_{(g)} + H_{2(g)} \xrightarrow{\text{slow}} N_2 + H_2O_2$
Step $2$: $H_2O_2 + H_2 \xrightarrow{\text{fast}} 2H_2O$
Then the correct statement is:
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View SolutionWhich of the following is a unimolecular reaction?
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