Half mole of an ideal monoatomic gas is heated at constant pressure of 1 atm from `20^(@)C " to " 90^(@)C`. Work done by gas is close to: (Gas constant R = 8.31 J/mol-K)

One mole of an ideal monoatomic gas is heated at a constant pressure of 1 atmosphere from 0^(@) C to 100^(@0 C. Work done by the gas is

One mole of an ideal monoatomic gas is heated at constant pressure from 0^@C to 100^@C . Calculate work done.

3.0 moles of ideal gas is heated at constant pressure from 27^(@)C to 127^(@)C . Then the work expansion of gas is

If one mole of an ideal gas with C_(v) = (3)/(2) R is heated at a constant pressure of 1 atm 25^(@)C to 100^(@)C . Which is correct

One mole of an ideal monatomic gas is heated at a constant pressure from 0^(@)C to 100^(@)C . Then the change in the internal energy of the gas is (given R = 8.32 J cdot mol cdot k^(-1))

Two moles of an ideal monatomic gas is heated at constant pressure so that its temperature increases from 127^° C to 227^° C , then work done by gas

Two moles of an ideal monatomic gas is heated at constant pressure so that its temperature increases from 127^° C to 227^° C , then work done by gas

Calculate DeltaU and DeltaH in calories if one mole of a monoatomic ideal gas is heated at constant pressure of 1 atm from 25^(@)C to 50^(@)C .

One mole of an ideal gas is heated at constant pressure of 1 atmosphere form 0^@C to 100^@C the change in the internal energy is (R = 8 J/ mol K )