for an ideal gas is . State whether the statement is true or false.
A
True
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B
False
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Solution
The correct option is A True
Derivation for the relation between and
At constant pressure and constant volume, the heat capacities are denoted by and respectively.
Therefore, the heat at constant pressure can be defined as: ; where is absolute temperature.
We know that in a chemical change, the released heat at constant pressure is defined as change in enthalpy.
Thus,
The heat at constant volume can be defined as:
We know that in a chemical change, the released heat at constant volume is defined as change in internal energy. Thus,
Now, for a mole of ideal gas, enthalpy is equal to the sum of internal energy and the product of pressure and volume: ; where is pressure and is volume.
The expression for change in these quantities will be:
From ideal gas equation, substituting in this expression:
is universal gas constant
Thus:
Substituting the values of and in the above expression, we get: