Difficult
The rate law for the reaction $RCl + NaOH_{(aq)} \to ROH + NaCl$ is given by $\text{Rate} = K_1[RCl]$. The rate of the reaction will be
- ADoubled on doubling the concentration of sodium hydroxide
- BHalved on reducing the concentration of alkyl halide to one half
- CDecreased on increasing the temperature of the reaction
- DUnaffected by increasing the temperature of the reaction
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Similar Questions
Which of the following statements is incorrect?
Easy
View SolutionFor the reaction $A + B \rightarrow \text{Product}$,the rate law is given by $\text{Rate} = K[A]^1[B]^2$. Which of the following statements is incorrect?
Easy
View SolutionWrite the differential rate expression for the following reactions and determine their order of reaction:
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
Medium
View SolutionFor the reaction $A + B \to \text{products}$,it is found that the rate of the reaction is proportional to the concentration of $A$,but it is independent of the concentration of $B$. Then:
Medium
View SolutionThe following data is given for the reaction between $A$ and $B$:
$S.NO.$ $[A] \ mol \ L^{-1}$ $[B] \ mol \ L^{-1}$ $Rate \ mol \ L^{-1} \ sec^{-1}$ $I$ $1 \times 10^{-2}$ $2 \times 10^{-2}$ $2 \times 10^{-4}$ $II$ $2 \times 10^{-2}$ $2 \times 10^{-2}$ $4 \times 10^{-4}$ $III$ $2 \times 10^{-2}$ $4 \times 10^{-2}$ $8 \times 10^{-4}$
Which of the following are correct statements?
$(a)$ Rate constant of the reaction is $1 \ mol^{-1} \ L \ sec^{-1}$.
$(b)$ Rate law of the reaction is $k[A][B]$.
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactants.
| $S.NO.$ | $[A] \ mol \ L^{-1}$ | $[B] \ mol \ L^{-1}$ | $Rate \ mol \ L^{-1} \ sec^{-1}$ |
| $I$ | $1 \times 10^{-2}$ | $2 \times 10^{-2}$ | $2 \times 10^{-4}$ |
| $II$ | $2 \times 10^{-2}$ | $2 \times 10^{-2}$ | $4 \times 10^{-4}$ |
| $III$ | $2 \times 10^{-2}$ | $4 \times 10^{-2}$ | $8 \times 10^{-4}$ |
Which of the following are correct statements?
$(a)$ Rate constant of the reaction is $1 \ mol^{-1} \ L \ sec^{-1}$.
$(b)$ Rate law of the reaction is $k[A][B]$.
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactants.
Difficult
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