The volume of a gas at `0^(0)C` is `546cc`. At constant pressure it is heated from `30^(0)C` to `50^(0)C` the change in volume is

A liter of air is heated from 27^(0)C to 177^(0)C at constant pressure. Final volume is

The volume of a gas at 20^(@)C is 100 CC at normal pressure when it is heated to 100^(@)C , its volume is 125 CC at the same pressure the volume coefficient of the gas is

4 moles of an ideal gas is at 0^(@) C . At constant pressure it is heated to double its volume, then its final temperature will be

One mole of an ideal gas for which C_(V)= 3//2R heated at a constant pressure of 1 atm from 25^(0)C "to" 100^(0)C What will be the amount of heat change at constant pressure?

3.0 moles of ideal gas is heated at constant pressure from 27^(@)C to 127^(@)C . Then the work expansion of gas is

When a gas is heated from 25^(@)C " to " 50^(@)C at constant pressure of 1 bar, its volume :

If V_(0) is the volume of a given mass of gas at 278 K at a constant pressure then according to Charle's law, the volume at 10^(@)C will be

If V_(0) is the volume of a given mass of gas at 278 K at a constant pressure then according to Charle's law, the volume at 10^(@)C will be