One mole of ideal gas is filled in `"2"` litre flask at `0^(@)C` ,the pressure of the gas will be

2.802 g of N_(2) gas is kept in one litre flask at 0^(@)C . Calculate the pressure exerted by the gas.

When 4 g of an ideal gas A is introduced into an evacuated flask kept at 25^(@)C , the pressure is found to be one atmosphere. If 6 g of another ideal gas B is then added to the same flask, the pressure becomes 2 atm at same temperature. The ratio of molecular weights (M_(A) : M_(B)) of the two gases would be

If 4 litre of H_(2) gas at 400 mm Hg and 47^(@)C is transferred to 19 litre flask at 107^(@)C . Then pressure of H_(2) gas is:

A vessel is filled with an ideal gas at a pressure of 10 atmospheres and temp 27^(0)C . Half of the mass of the gas is removed from the vessel the temperature of the remaining gas is increased to 87^(0)C . Then the pressure of the gas in the vessel will be

A flask is filled with 13 g of an ideal gas at 27^(@)C and its temperature is raised to 52^(@)C . The mass of the gas that has to be released to maintain the temperature of the gas in the flask at 52^(@)C , the pressure remaining the same is

The K.E. of one mole of an ideal gas is

In an isothermal expansion of one mole of an ideal gas against vacuum from 10 litre to 100 litre at 27^(@)C , the quantity of heat absorbed by the gas is