Molar heat capacity of an ideal gas at constant volume is given by `C_(V)=2xx10^(-2)J` (in Joule). If 3.5 mole of hits ideal gas are heated at constant volume from 300K to 400K the change in internal energy will be

A gas of volume changes 2 litre to 10 litre at constant temperature 300K, then the change in internal energy will be :

A gas of volume changes 2 litre to 10 litre at constant temperature 300K, then the change in internal energy will be :

One mole of a gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is:

One mole of a gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is :-

One mole of a gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is :-

The constant volume molar heat capacity of an ideal gas is expressed by C_(v, m) = 16.5 +10^(-2)T (All values are in SI units). If 2.5 mol of this gsa at constant value is heated from 27^(@)C ro 127^(@)C , the internal energy increases by ''x'' kJ. Hence, x is

The molar specific heat of a gas at constant volume is 24 J/mol ^@K . Then change in its internal energy if one of such gas is heated at constant volume from 10^@C to 30^@C is

When two mole of an ideal gas (C​_(p.m.) = 5/2R) heated from 300K to 600K at constant volume. The change in entropy of gas will be :-

The molar specific heat of a gas at constant volume is 24 J/mol K. then change in its internal energy if one mole of such gas is heated at constant from 10^(@)C to 30^(@)C is