A gas is kept in a closed containers at constant temperature. Keeping the temperature constant if some amount of the gas is incorporated.what will be the change in pressure?

If a gas expands at constant temperature.

If a gas expand at constant temperature :

Isothermal (temperature=constant) graphs of a gas is its

For an ideal gas, C_(V)=(3)/(2)R . (a) What will be the change in internal energy (DeltaU) of 1 mole of an ideal gas if its temperature is increased by 4K at constant volume ? What would be DeltaU if the temperature of this gas is increased by the same amount of constant pressure? keeping pressure constant if the temperature of that same amount of gas is increased by 4K then what will be the change in internal energy (DeltaU) of that gas? (c) give reason for different values of DeltaU and DeltaH ?

If a gas expands at a constant temperature it indicates that

At constant pressure, if the temperature of gas is increased then its density-

A certain amount of an ideal gas is enclosed in a cylinder fitted with a movable piston. What would be the changes of the volume of the gas in the following processes? (i) The pressure of the gas is reduced by 25% at constant temperature. (ii) The temperature of the gas is increased by 50% constant pressure.

The following changes are performed on 1 mol of N_(2) gas- (i) Pressure is decreased at constant at constant temperature. (ii) volume is decreased at constant temperature. What will be the sign of DeltaS_(sys) in these changes?

(i) The pressure and temperature of 0.8 g of He gas are 1 atm and 298 K respectively. If 400 J of heat is applied to the gas at constant volume, what will be change in internal energy and the final temperature of the gas ? (ii) If the same amount of heat is applied to the gas at constant pressure, then what will be the change in internal energy and the final temperature of the gas ? For both the cases, assume He gas behaves ideally and its C_(V)=(3)/(2)R .