`40` g of Argon is heated from `40^(@)C` to `100^(@)C (R=2 cal//mol.)` What is the heat absorbed at the constant volume by the Argon?

When gases are heated from 20^(@) to 40^(@) C at constant pressure their volumes

5' moles of oxygen is heated at constant volume from 10^(@)C to 20^(@)C . What will be the change in the internal energy of the gas in calories? (For the gas C_(P)=7cal//gm" "mol//.^(@)C&R=2cal//mol" ".^(@)C )

How much heat energy should be added to the gaseous mixture consisting of 1 g of hydrogen and 1g of helium to raise it s temperature from 0^(@)C to 100^(@)C (a) at constant volume, b. at constant pressure (R = 2 cal//mol K) ?

How much heat energy should be added to the gaseous mixture consisting of 1 g of hydrogen and 1g of helium to raise it s temperature from 0^(@)C to 100^(@)C (a) at constant volume, b. at constant pressure (R = 2 cal//mol K) ?

Six moles of O_(2) gas is heated from 20^(@)C to 35^(@)C at constant volume . If specific heat capacity at constant pressure is 8 " cal mol"^(-1)-K^(-1) and R=8.31"J mol"^(-1)-K^(-1) , what is change in internal energy of gas ?

70 calorie of heat is required to raise the temperautre of 2 mole of an ideal gas at constant pressure from 40^(@)C to 45^(@)C. Find the amount of heat required to raise the temperature of the same through the same range at constant volume (R = 2 cal/mol-K)

Suppose that 5 g of helium gas is heated from -30^@C to 120^@C . Find its change in internal energy and the work it does if the heating occurs (a) at constant volume and (b) at constant pressure. For helium, C_v =0.75 cal/g. C^@ and C_p =1.25 cal/g . C^@