Medium
For a certain reaction,the rate $= k[A]^2[B]$. When the initial concentration of $A$ is tripled keeping the concentration of $B$ constant,the initial rate would:
- AIncrease by a factor of $3$
- BDecrease by a factor of $9$
- CIncrease by a factor of $6$
- DIncrease by a factor of $9$
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Similar Questions
For a certain reaction,the rate constant $K = 2.37 \times 10^2 \ L^2 \ mol^{-2} \ s^{-1}$. What is the order of the reaction?
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 SolutionIdentify the correct statement regarding the order of reaction from the following.
Write the differential rate expression for the following reaction and determine its order of reaction:
$H_{2}O_{2} + I^{-} \rightarrow H_{2}O + IO^{-}$
$H_{2}O_{2} + IO^{-} \rightarrow H_{2}O + I^{-} + O_{2}$
$H_{2}O_{2} + I^{-} \rightarrow H_{2}O + IO^{-}$
$H_{2}O_{2} + IO^{-} \rightarrow H_{2}O + I^{-} + O_{2}$
Medium
View SolutionFor the reaction $NO_2 + CO \rightarrow CO_2 + NO$,the rate law is given as $\text{Rate} = K [NO_2]^2$. What is the number of $CO$ molecules participating in the slow step?
Easy
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