5 moles of oxygen are heated at constant volume from `10^@C` ot `20^@C`.What will be the change in the internal enregy of the gas?The molar specific heat of oxygen at constant pressure is `C_p=7.03 cal mol^(-1) deg^-1` and `R=8.36 Joule mol^(-1) "^oC^(-1)`.

0.32 g of oxygen is kept in a rigid container and is heated .Find the heat energy needed to raise the temperature from 25^@C to 35^@C .The molar heat capacity of oxygen at constant volume is 20 J mol^(-1) K^(-1) .

Temperature of 1 mole of a gas is increased by 2^(@)C at constant pressure. Work done is :

Calculate the difference between the two specific heats of Helium gas per gram. Given that molecular weight of He = 4, J = 4.18 joule/cal and R = 8.31 J mole^-1//K^-1 ?

The molar heat capacity of a gas at constant volume is to be 5 cal mol^(-1) K^(-1) .Find the ratio gamma=C_p // C_v for the gas.The gas constant R=2 cal mol^(-1) K^(-1) .

The osmotic pressure of 0.2 molar solution of urea at 27^@C (R=0.082 litre atm "mol"^(-1) K^(-1)) is

The standard enthalpy of formation of gaseous H_(2)O at 298 K is -241.82 kJ/mol. Calculate DeltaH^(@) at 373 K given the following values of the molar heat capacities at constant pressure : H_(2)O(g)=33.58 " JK"^(-1)" mol"^(-1), " "H_(2)(g)=29.84 " JK"^(-1)" mol"^(-1), " "O_(2)(g)=29.37 " JK"^(-1)" mol"^(-1) Assume that the heat capacities are independent of temperature :

A sample of gas occupies 1.50L at 25 o C. If the temperature is raised to 60 o C, what is the new volume of the gas if pressure remains constant?

What amount of heat must be supplied to 2.0 xx 10^-2 kg of nitrogen (at room temperature) to raise its temperature by 45 ^@C at constant pressure ? (Molecular mass of N_2 = 28, R = 8.3 J mol^-1 K^-1. )