Find out the temperature in `.^@C` at which 0.225 mole of oxygen will occupy a volume of 6000 mL at 560 mm pressure.Given : R = 0.082 lit. atm `(mol e-k)^-` .

Determine the pressure of 4.032 g of Hydrogen occupying 16.8 litres of volume at 0^@C (R=8.315 J/mol K)

At what temperature would the volume of a given mass of a gas at constant pressure be twice to its volume at 0^@C

Vapour density of a gas is 32. Find the volume of 0.64 g gas at 27^@ C and 684 mm pressure .

The gas phase decomposition of dimethyl ether follows the first order kinetics as CH_3 - O - CH_(3) (g) to CH_(4) (g) + H_(2) (g) + CO(g) This reaction is carried out in a constant volume container at temperature of 500°C and has a half-life of 14.5 min. Initially, only dimethyl ether is present at a pressure of 0.40 atm. After 12 min, find the total pressure of the system. Assume ideal gas behaviour.

At 27^@C , the osmotic pressure of a solution containing 4.0 g solute (molar mass = 246 ) per litre at 27^@C is : R = 0.0821 atms. mol^-1 k )

The density of H_2 at 0^@ C and 760 mm pressure is 0.00009 g/cc. Find te R.M.S velocity of H_2 molecules.

When the temperature of a reaction is raised from 47°C to 57°C, the rate of the chemical reactions is doubled. Calculate the E_a . (Given, R = 8.314"J mol"^(-1)" K"^(-1) )

200 Ml of a gas had a temperature 27^@ C and pressure 750 mm. Find the pressure at which the gas will have a volume 175mL if the temperature is 77^@ C .

What amount of heat must be supplied to 2.0xx10^(-2) kg of nitrogen at room temperature to raise it's temperature by 45^@C at constant volume ? Given molecular weight of N_2 is 28 and R=8.3 J mol^(-1)k^(-1) and C_V (diatomic gases)= 7/2 R