**∆G° = – RT ln K ……(1)**

**∆G° = ∆H° – T∆S° -(2)**

**– RT ln K = ∆H° – T∆S°**

**ln K = − Δ H °/R T + T ΔS °/R T**

**ln K = − Δ 𝐻 °/ 𝑅 𝑇 + Δ 𝑆 °/ 𝑅 ….(3)**

**Equation is known as integrated form of van't Hoff equation.**

Showing posts with label **CHEMICAL KINETICS**. Show all posts

Showing posts with label **CHEMICAL KINETICS**. Show all posts

This equation gives the quantitative temperature dependance of equilibrium constant K.

**∆G° = – RT ln K ……(1) ****∆G° = ∆H° – T∆S° -(2) **

**– RT ln K = ∆H° – T∆S° **

**ln K = − Δ H °/R T + T ΔS °/R T****ln K = − Δ 𝐻 °/ 𝑅 𝑇 + Δ 𝑆 °/ 𝑅 ….(3) **

**Equation is known as integrated form of van't Hoff equation.**

The relation between standard free energy change ∆G° and equilibrium constant is

We know that,

Substituting (1) in equation (2)

Rearranging,

Differentiating equation (3) with respect to temperature

d(in K) = d(in K) / dT = ∆H° / RT2

Equation (4) is known as differential form of van't Hoff equation.

On integrating the equation (4), between T1 and T2 with the respective equilibrium constants and K2

Vapour pressure is directly proportional to the Temperature so that on increasing temperature the rate of evaporation increases and rate of condensation decreases and hence vapour pressure increases.

**Arrhenius equation:**

The temperature
dependence of rate of a chemical reaction can be accurately explained by
Arrhenius equation. It was first proposed by Dutch chemist J.H.
Vant’s Hoff but Swedish chemist Arrhenius
provides its physical justification and interpretation.

**Where**

K=
Rate constant

**A= **Arrhenius constant or frequency
factor or pre exponential factor

**R=** Universal gas constant =25/3 joule
per mole per second

**Ea=** Activation
Energy

**T=** temperature

**-Ea/RT=** Boltzmann factor or fraction of molecule having equal **or** greater
than Activation energy **or** fraction of molecule that have
kinetic energy greater than activation energy.

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Book
by O.P Tandon

(2) Physical chemistry

Book by KS Verma (Cengage
Publications)

(3) Physical Chemistry

Book by P.W. Atkins (Oxford publication)

(4) Physical Chemistry

Book by P. Bahadur

(5) Physical Chemistry

Book by Ranjeet
Shahi (Arihant publication)

(6) Balaji Advanced problems
in Physical chemistry

Book by Narendra
Awasthi

(7) Modern
Approach to Chemical Calculations

Book by R.C. Mukherjee

The temperature
dependence of rate of a chemical reaction can be accurately explained by
Arrhenius equation. It was first proposed by Dutch chemist J.H.
Vant’s Hoff but Swedish chemist Arrhenius
provides its physical justification and interpretation.

**Where**

K=
Rate constant

**A= **Arrhenius constant or frequency
factor or pre exponential factor

**R=** Universal gas constant =25/3 joule
per mole per second

**Ea=** Activation
Energy

**T=** temperature

**-Ea/RT=** Boltzmann factor or fraction of molecule having equal **or** greater
than Activation energy **or** fraction of molecule that have
kinetic energy greater than activation energy.

Related Questions:

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