Why different gases have different heat capacity ratio values?

Expert Solution

when any gaseous system is maintained at a constant pressure and in this condition if heat energy is supplied , then the given energy will increases the temperature of the gas. The total energy of a given number of moles of gas at any particular given temperature is equals to nRT, from the Ideal Gas Equation of State, where n stands for the number of moles of gas particles, R is the universal gas constant, and T is the temperature of the gas. However, it is observed that some gases will have a larger temperature increase when we compared to it with other gases for the same amount of energy input requirement , or, in other words we can say that they have different specific heat capacities.

First there occcurs a translational motion. That accounts for the value of 3/2 R. All gases possess that.

Next comes the rotational energy. Monoatomic gases don't possess that because they don't possess any rotational levels. If gases are linear, gase have R, if gas are non-linear, gas will have 3/2 R.

Then you'll have what is called vibrational energy. That can add up to (3n-5)/2 R for linear molecule and (3n-6)/2 R for non-linear molecules. The n is the number of atoms.

therefore all the heat always used towards increasing the temperature of the system (maintained at constant volume and at constant pressure then there's always a part which will becomes expansion work); the difference between these gases will be given by their different specific heat.

Amanda K answered 2 years ago

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