Question

Molar heat capacity of a gas does not depend on:
A.Its temperature
B.Its molecular weight
C.Its atomicity
D.The condition under which heat is supplied

Answer 1

Hint:Molar heat capacity depends on the number of atoms present in a molecule and whether the system is adiabatic or not. It is the amount of heat to be supplied to one mole of substance to increase its temperature by 1 unit.

Complete answer:
When a hot body is placed in contact with a cold one, the former gets colder and the latter gets warmer. Certain amount of heat has passed from the hot body to the cold body. Heat is a form of energy. Heat is felt by its effect of change in degree of hotness, expansion of body, change in state and etc. SI unit of heat is joule or J. Heat is also measured in unit calorie. A calorie is defined as the amount of heat required to raise the temperature of a \[1{\text{g}}\] water by \[1^\circ {\text{C}}\] or \[1{\text{K}}\] . \[4.2{\text{joule}}\] is equivalent to one calorie of energy or heat.
Specific heat is the amount of energy required to raise the temperature of a unit mass of substance by \[1^\circ {\text{C}}\] or \[1{\text{K}}\] . It is represented by s or c. It depends on the pressure, volume and temperature of substance. For liquids and solids, specific heat is most often made at a constant pressure as functions of temperature, because constant pressure is quite easy to be maintained experimentally.
Molar heat capacity is defined as the amount of energy required to raise or increase the temperature of one mole of a given substance by \[1^\circ {\text{C}}\] or \[1{\text{K}}\] is called as molar heat capacity. The molar heat capacity is the product of molecular weight and specific heat as per follow: \[{\text{Molar heat capacity C}} = {\text{molecular weight}}\left( {\text{M}} \right) \times {\text{specific heat}}\left( {\text{c}} \right)\] and it can also be written as in terms of moles and heat exchange and change in temperature:
\[{\text{C}} = \dfrac{1}{\mu }\left( {\dfrac{{{\text{dQ}}}}{{{\text{dT}}}}} \right)\] .
Molar heat capacity can be written as in terms of mass m and molar mass M of a substance as: \[{\text{C}} = \dfrac{{\text{M}}}{{\text{m}}}\left( {\dfrac{{{\text{dQ}}}}{{{\text{dT}}}}} \right)\] .
Molar heat capacity depends on whether the heat is added at constant pressure or constant volume and nature of gas including its atomicity. It does not depend on temperature and amount of substance because it is defined to increase the temperature by \[1^\circ {\text{C}}\] or \[1{\text{K}}\] for one mole of a substance.

Thus, the correct options are A and B.
Note:
Heat capacity is the amount of heat required to raise the temperature of the whole substance through \[1^\circ {\text{C}}\] or \[1{\text{K}}\] , it depends on property of substance and also mass of the body.