Heat capacity `(C_(V))` of an ideal gas is X KJ/mole/K. To rise its temperature from 298 K to 318 K, heat to be supplied per 10g gas will be (in KJ) [MW = 16]

The molar specific heat capacity at constant volume (C_(V)) for an ideal gas changes with temperature as shown in the graph. Find the amount of heat supplied at constant pressure in raising the temperature of one mole of the gas from 200 K to 400 K.

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 :-

Molar heat capacity (C_(p)) of water of constant pressure is 75JK^(-1) mol^(-4) . The increase in temperature (in K) of 100g of water when I kJ of heat is supplied to it is

One mole of an ideal gas requires 207 J heat to rise the temperature by 10 K when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same 10 K , the heat required is (Given the gas constant, R = 8.3 J/mol-K).