The rate law for the reaction$RCl + NaOH(aq) \to ROH + NaCl$ is given by Rate $ = {K_1}[RCl]$. The rate of the reaction will be
The rate law for the reaction$RCl + NaOH(aq) \to ROH + NaCl$ is given by Rate $ = {K_1}[RCl]$. The rate of the reaction will be
- [IIT 1988]
- A
Doubled on doubling the concentration of sodium hydroxide
- B
Halved on reducing the concentration of alkyl halide to one half
- C
Decreased on increasing the temperature of the reaction
- D
Unaffected by increasing the temperature of the reaction
Similar Questions
Consider a reaction $\mathrm{aG}+\mathrm{bH} \rightarrow$ Products. When concentration of both the reactants $\mathrm{G}$ and $\mathrm{H}$ is doubled, the rate increases by eight times. However, when concentration of $\mathrm{G}$ is doubled keeping the concentration of $\mathrm{H}$ fixed, the rate is doubled. The overall order of the reaction is
Consider a reaction $\mathrm{aG}+\mathrm{bH} \rightarrow$ Products. When concentration of both the reactants $\mathrm{G}$ and $\mathrm{H}$ is doubled, the rate increases by eight times. However, when concentration of $\mathrm{G}$ is doubled keeping the concentration of $\mathrm{H}$ fixed, the rate is doubled. The overall order of the reaction is
- [IIT 2007]
Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?
Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?
Consider the following gas-phase reaction.
$2HI(g) \longrightarrow H_2(g) + I_2(g)$
and the following experimental data obtained at $555\, K$, What is the order of the reaction with respect to $HI$ $(g)$ ?
$[HI]$, $M$
rate, $Ms^{-1}$
$0.0500$
$8.80 \times {10^{ - 10}}$
$0.1000$
$3.52 \times {10^{ - 9}}$
$0.1500$
$7.92 \times {10^{ - 9}}$
Consider the following gas-phase reaction.
$2HI(g) \longrightarrow H_2(g) + I_2(g)$
and the following experimental data obtained at $555\, K$, What is the order of the reaction with respect to $HI$ $(g)$ ?
| $[HI]$, $M$ | rate, $Ms^{-1}$ |
| $0.0500$ | $8.80 \times {10^{ - 10}}$ |
| $0.1000$ | $3.52 \times {10^{ - 9}}$ |
| $0.1500$ | $7.92 \times {10^{ - 9}}$ |
Why is the probability of reaction with molecularity higher than three very rare ?
Why is the probability of reaction with molecularity higher than three very rare ?
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$