At `27^@C` temperature a gas occupies 2L. In which temperature at constant pressure it will occupy 3L.

At 27^@C temperature and 760 mm of Hg pressure a certain quantity gas occupies 1000cc. At what temperature at 750 mm of Hg pressure gas will occupy 1520 cc.

A certain quantity air occupies 1000cm^3 at 20^@C temperature and 760 mm Hg pressure. At what temperature and 750 mm Hg pressure it will it will occupy 1400 cm^3?

The temperature of an ideal gas is 340 K. the gas is heated to a temperature at constant pressure. As a result, its volume increases by 18%. What is the final temperature of the gas?

At 760 mm of Hg pressure of 0^@C temperature a gas occupies 300 cm^3 . What will be the volume at 546^@C at same pressure.

At 273 K and 76 cm pressure, the volume of 0.64 g of any gas is 224 mL. At what temperature 1 g of that gas at 1 atm pressure will occupy a volume of 1 litre?

How does the density of a given mass of a gas vary with temperature at constant pressure?

Volume of a gas is doubled by raising its temperature at constant pressure . Initial temperature of the gas was 13^@C . Find the final temperature.

A gas occupies 750cc at - 3^@ C . Under same pressure at what temperature the gas will occupy 1 L.

A fixed mass of gas occupies a volume of 273 cm^3 at STP. At what pressure the above gas will occupy a volume of 300 cm^3 at 27^@C ?