Iron react with HCl at `25^@C` & 1 bar pressure & give `FeCl_2` & `H_2`(g), then find magnitude of work done (in KJ) in this process at 1 bar constant pressure

Temperature of 1mol of a gas is increased by 1^(@) at constant pressure. The work done is

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

A balloon is 1m in diameter and contain air at 25^(@)C and 1 bar pressure. It is filled with air isothermally and reversibly until the pressure reaches 5bar. Assume pressure is propotional to diameter of ballon. Calulate work done by air (atm ,m^(3))

At 25^(@)C , 50 g of iron reacts with HCl to form FeCl_(2) . The evolved hydrogen gas expands against a constant pressure of 1 bar. The work done by the gas during this expansion is (Round off to the Nearest Integer). [Given : R=8.314 J mol^(-1)K^(-1) . Assume, hydrogen is an ideal gas] [Atomic mass of Fe is 55.85 u]

A system consisting of 1 mole of an ideal gas undergoes an isothermal expansion at 25^(@) from 1.0 bar to a lower pressure while generating 100 J of work. What is the final pressure of the system if the external pressure of the system is constant of 0.1 bar?

Temeprature of 1 mole of a gas is increased by 2^(@) at constant pressure, then work done is :

The density of CO_(2) is 0.326 g dm^(-3) at 27^(@)C and 0.25 bar pressure. What is the density of the gas at 47^(@)C keeping the pressure constant?

What will be the work done for expansion of a gas from 1 lit to 10 lit volume agaist constant pressure of 1 bar?