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Third Law of Thermodynamics

Vant Hoff's e...

Question

Vant Hoff's equation is ___.

A

l o g \frac{K_{2}}{K_{1}} = \frac{- Δ H^{0}}{2.303 R} [\frac{T_{2} - T_{1}}{T_{2} T_{1}}]

.

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B

l o g \frac{K_{2}}{K_{1}} = \frac{Δ H^{0}}{2.303 R} [\frac{T_{2} - T_{1}}{T_{2} + T_{1}}]

.

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C

l o g \frac{K_{2}}{K_{1}} = \frac{Δ H^{0}}{2.303 R} [\frac{T_{2} - T_{1}}{T_{2} T_{1}}]

.

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D

l o g \frac{K_{2}}{K_{1}} = \frac{Δ H^{0}}{2.303 R} [\frac{T_{2} + T_{1}}{T_{2} T_{1}}]

.

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Solution

The correct option is C $l o g \frac{K_{2}}{K_{1}} = \frac{Δ H^{0}}{2.303 R} [\frac{T_{2} - T_{1}}{T_{2} T_{1}}]$ .
The van't Hoff equation provides information about the temperature dependence of the equilibrium constant. The van't Hoff equation may be derived from the Gibbs-Helmholtz equation, which gives the temperature dependence of the Gibbs free energy.

The van't Hoff equation is $K = A e^{Δ H / R T}$ or $\frac{d l n K}{\partial T} = \frac{Δ H}{R T^{2}}$

By, integrating the above equation, you will get the required relation.

Hence, the given statement is correct

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Similar questions

Q. For a reversible reaction

a A + b B ⇌ c C + d D

; the variation of

K

with temperature is given by

log \frac{K_{2}}{K_{1}} = \frac{- Δ H^{o}}{2.303 R} [\frac{1}{T_{2}} - \frac{1}{T_{1}}]

Q. The effect of temperature on equilibrium constant is expressed as

(T_{2} > T_{1})

l o g \frac{K_{2}}{K_{1}} = \frac{- Δ H}{2.303} [\frac{1}{T_{2}} - \frac{1}{T_{1}}]

. For endothermic reaction false statement is:

Q. Vant' Hoff equation shows the effect of temperature on equilibrium constants

K_{c}

K_{p} .

K_{p}

varies with temperature according to the relation:

Q. Effect of increasing temperature on equilibrium constant is given by

l o g K_{2} - l o g K_{1} = \frac{- Δ H}{2.303 R}

[\frac{1}{T_{2}} - \frac{1}{T_{1}}]

. Then for an endothermic reaction the false statement is:

Q. Match the column I with column II and mark the appropriate choice.

Column I	Column II
(A) Zero order	(i) $log \frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303 R} [\frac{T_{2} - T_{1}}{T_{1} T_{2}}]$
(B) First order	(ii) $Δ H > 0$
(C) Endothermic reaction	(iii) $k = \frac{2.303}{t} log \frac{[A]_{0}}{[A]}$
(D) Activation energy	(iv) $k = \frac{1}{t} ([A]_{0} - [A])$

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