Rate law for the following reaction- Ester-H- Acids- Alcohol- is dx-dt-k -ester-1 -H-0- What would be the effect on the rate if concentration of H- ion is doubled-

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Standard XII

Chemistry

Physical Properties of Alkenes

Rate law for ...

Question

Rate law for the following reaction; $E s t e r + H^{+} ⇌ A c i d s + A l c o h o l$ ; is $\frac{d x}{d t} = k [e s t e r]^{1} [H^{+}]^{0}$ . What would be the effect on the rate if concentration of $H^{+}$ ion is doubled?

Same

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Doubled

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Half

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Data insufficient

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Solution

The correct option is A Same
As reaction does not depend on the concentration of $H^{+}$ , therefore, rate will be the same.

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Similar questions

Q. The rate law for the reaction :

E s t e r + H^{+} \to A c i d + A l c o h o l

V = k [e s t e r] {[H_{3} O^{+}]}_{3}^{0}

What would be the new rate if
(a)

conc. of ester is doubled
(b)

conc. of

H^{+}

is doubled

Q. For acid catalysed hydrolysis of ester rate law obtained is rate

= [e s t e r] [H^{+}],

where

k = 0.01 M^{- 1} {h r}^{- 1} .

What is the half-life if the initial concentrations are

0.02 M

for the ester and

0.05 M

for the catalyzing acid?

$Z n + 2 H^{+} \to Z n^{2 +} + H_{2}$

Half – life period is independent of concentration of constant pH. For the constant concentration of Zn, rate becomes 100 times when pH is decreased from 3 to 2. Hence,

H_{2} + {B r}_{2} \to 2 H B r

The rate law is

\frac{d x}{d t} = k [H_{2}]^{1 / 2} {[{B r}_{2}]}^{1 / 2}

On increasing the concentration of

{B r}_{2}

four times, by how much times the rate of reaction will change?

Q. Which of the following statement is true for the reaction,

H_{2} + {B r}_{2} \to 2 H B r

. The rate law is

\frac{d x}{d t} = k [H_{2}] {[{B r}_{2}]}^{1 / 2}

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Rate law for the following reaction; Ester+H+⇌Acids+Alcohol; is dxdt=k[ester]1[H+]0. What would be the effect on the rate if concentration of H+ ion is doubled?

The correct option is A SameAs reaction does not depend on the concentration of H+, therefore, rate will be the same.

Rate law for the following reaction; $E s t e r + H^{+} ⇌ A c i d s + A l c o h o l$ ; is $\frac{d x}{d t} = k [e s t e r]^{1} [H^{+}]^{0}$ . What would be the effect on the rate if concentration of $H^{+}$ ion is doubled?

The correct option is A Same
As reaction does not depend on the concentration of $H^{+}$ , therefore, rate will be the same.