If `N_2` is bubbled through water at 293 K, how many milli moles of `N_2` gas would dissolve in 1 litre of water. Assume that `N_2` exerts a partial pressure of 0.987 bar. Given that Henry's law constant for `N_2` at 293 K is 76.48 k bar.

A mixture of N_(2) and O_(2) at 1 bar pressure contains 80% N_(2) by weight. Calculate the partial pressure of N_(2) in the mixture.

The product of volume and pressure of how many gram of N_2 gas is 244 litre atmosphere at STP?

Calculate the concentration of CO_2 in a soft drink that is bottled with a partial pressure of CO_2 of 4 atm over the liquid at 25^@C . The Henry's Law constant for CO_2 in water is 3.1 xx 10^-2 mol/litre atm at 25^@C .

A gas mixture was prepared by taking equal mole of CO and N_(2) . If total pressure of the mixture was 1 atm, the partial pressure of N_(2) in the mixture is-

A gaseous mixture was prepared by taking equal moles of CO and N_2 . If the total pressure of the mixture was found 1 atm, the partial pressure of the nitrogen (N_2) in the mixture is

A mixture of F_(2) gas and an excess of xenon gas is heated at 673K under a pressure of 1 bar.

Assuming that water vapour is an ideal gas, the internal energy change (DeltaU) when 1 mol of water is vaporised at 1 bar pressure and 100^(@)C , will be (Given: at 1 bar and 373 K, molar enthalpy of vaporisation of water is 41kJ*mol^(-1),R=8.3J*mol^(-1)*K^(-1) )-

A mixture containing N_2 and H_2 in a mole ratio 1 : 3 is allowed to attain equilibrium when 50% of the mixture has reacted. If P is the pressure at equilibrium, then the partial pressure of NH_3 formed is