When the tempeature of 10 g of an enclosed gas is raised by `50^@C`, the gas expands by 2.5 litres against normal atmospheric pressure.
The sp. ht. at constant volume for the gas is `0.8 kcal//kg//K`. Calculate the heat supplied. `J =4200 J//k` cal.

A gas is heated from 0^@ C to 100^@ C at 1.0 atm pressure. If the initial volume of the gas is 10 litre, its final volume would be :

Specific heats of Nitrogen at constant pressure and at constant volume are 0.216 and 0.175 cal/mol/K respectively.Given R = 8.31 J/mol K. Calculate the mechanical equivalent of heat.

When 1.3 g of a solute is dissolvedf in 169 g of water the boiling point of the solution is 100.025^@C at one atmospheric pressure. If K_b of water is 0.52 K kg mol^(-1) . Calculate the molecular mass of the solute.

When 80 litres of a gas at 27^@C and 10 atmospheres is reduced to 50 litres by increasing the pressure, the temperature increases to 37^@C . What is the final pressure on the gas assuming it to be ideal ?

What volume of hydrogen gas measured at 273 K at 0.5 atmospheric pressure will be obtained when 0.1 faraday of electricity is passed through acidulated water ?

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:

Two elements A and B form compounds having molecular formula AB_(2) and AB_(4) When dissolved in 20 g of benzene, 1 g of AB_(2) lowers the freezing point by 2.3 K, whereas 1.0 g of AB_(4) lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol^-1 . Calculate the atomic mass of A and B.