The rate of the reaction $CCl_3CHO + NO \to CHCl_3 + NO + CO$ is given by $Rate = K [CCl_3CHO] [NO]$. If concentration is expressed in $mol \ L^{-1}$,the units of $K$ are:
- A$L^2 \ mol^{-2} \ s^{-1}$
- B$mol \ L^{-1} \ s^{-1}$
- C$L \ mol^{-1} \ s^{-1}$
- D$s^{-1}$
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The 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:
Difficult
View SolutionWhich of the following is an example of a second-order reaction?
In the reaction $2A + B \to A_2B$,if the concentration of $A$ is doubled and the concentration of $B$ is halved,then the rate of the reaction will:
For the reaction $A + 2B \to C$,the rate equation is given as $\text{Rate} = K[A][B]$. If the concentration of $A$ is kept constant but that of $B$ is doubled,what will happen to the rate of the reaction?
DifficultJEE MAIN 2015
View SolutionFor a chemical reaction,which of the following can never be a fraction?
Easy
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