At constant pressure, a fixed mass of a gas is heated form `0^@C` to `30^@C`. Find the ratio of the volumes of the gas at `0^@C` and `30^@C`.

At constant pressure, the temperature of a difinite amount of a gas is increased from 0^(@)C to t^(@)C . As a result, the volume of the gas is increased by a factor of three. Calculate the value of t.

At constant pressure if the temperature of 5L of a gas is increased from 0^@C to 35^@C the volume increases by 640 cm^3 From this data,determine the value of absolute zero temperature is Celsius scale.

IF heated to 35^@C at constant pressure, the volume of gas increases from 5L to 0^@C by 640 cm^3 . What should be the value of absolute zero for this gas in Celsius scale?

IF 2 mol of a gas at constant pressure, requires 70 cal heat to increase its temperature from 30^@C to 35^@C , then find its degrees of freedom.

Volume of a gas at STP is 10 L. What will be the volume of the gas at 27^@C and 750 mm pressure?

Plot density vs pressure for a fixed mass of an ideal gas at a constant temperature.

70 cal of heat is required to raise the temperature of 20 moles of an ideal diatomic gas at constant pressure from 30^@C . The amount of heat required (in cal) to raise the temperature of the same gas through the same range ( 30^@C to 35^@C ) at constant volume is

A certain mass of a gas occupies 100 cc at 50^@C . Its volume at 0^@C is-

At constant pressure if the volume of a fixed mass of gas at temperature 80^@C is 500cm^3 and that at 150^@C is 600cm^3 , what is the coefficient of volume expansion (gamma_p) of the gas?

10 mol of an ideal gas is taken through an isothermal process in which the volume is compressed from 40 L to 30 L. If the temperature and the pressure of the gas are 0^(@)C and 1 atm respectively. Find the work done in the process. Given: R = 8.31 J cdot mol^(-1) cdot K^(-1) .