Chemistry, asked by aasthakansal7646, 1 year ago

The molar specific heat at constant volume of an ideal gas is equal to 2.5 times the universal gas constant (8.314 j/mol k). When the temperature increases by 100 k, the change in molar specific enthalpy is

Answers

Answered by deepureddy1810
0

In general specific heat(C)  gives us an idea of the amount of energy(heat) we need to provide to a system in order to bring about a unit rise in the temperature of the system. It's value may vary depending on the process you are providing this energy. Hence we have two values of C namely Cv and Cp .

Cv for a gas is the change in internal energy (U) of a system with respect to change in temperature at a fixed volume of the system i.e. Cv =(∂ U/∂ T)v whereas Cp for a gas is the change in the enthalpy (H) of the system with respect to change in temperature at a fixed pressure of the system i.e Cp= (∂ H/∂ T)p.

We know that, ΔH = ΔU + PΔV (+ VΔP, ΔP=0 for constant pressure) . So the enthalpy term is  greater than the internal energy term because of the PΔV term i.e in case of a constant pressure process more energy is needed, to be provided to the system as compared to that of a constant volume process to achieve the same temperature rise, as some energy is utilized in the expansion work of the system. And the relation that correlates these two is Cp = Cv + R

But since liquids and solids can practically assumed to be incompressible, Cp and Cv for them have almost same values and hence only a single value of specific heat is used for them.

Here is the answer to your question:

    Cp=3.5R.

Cv=Cp-R=2.5R. Ratio=3.5/2.5=7/

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