The solubilling of `N_2` gas in water at `25^@C` and 1 bar is `6.85xx10^(-4)` mol `L^(-1)`. Calculate henry's law constant Molarity of `N_2` gas dissolved in water under atmospheric conditions when partial pressure of `N_2` in atmosphere is 0.75 bar.

The solubility of nitrogen gas at1bar pressure at 25^@C is 6.8 xx 10^(-4) moldnr^(-3 . Calculate the solubility of N_2 gasfrom atmosphere at 25^@C if atmospheric pressure is 1 bar and partial pressure of N_2 gas at this temperature and pressure is 0.78 bar.

The solubility of nitrogen gas at 2 atm pressure at 25^(@)C " is " 13.6xx10^(-4) mol dm^(-3) calculate the solubility of N_(2) gas from atmosphere at 25^(@)C, of atmospgeric pressure is 2 atmosphere and partial pressure of N_(2) gas at this temperature and pressure is 1.53 atm.

The density of a gas at 27^@C and 1 bar pressure is 2.56 gL^-1 .Calculate the molar mass.

A mixture of 28 g N_2 and 16 g He has 25 bar pressure. The partial pressure of N_2 in the mixture is ____ bar.

For a gas the Henry's law constant is 1.25xx10^(-3) mol dm^(-3) bar .^(-1) at 50^@C . Calculate the solubility of the given gas at 5 bar and 50^@C ,.

The solubility of oxygen gas at 25^(@)C at 1 atmosheric pressure is 1.43 xx10^(-4) mol dm^(-3) Calculate the partial pressure of oxygen if the Henry's law constant for oxygen is 0.65 xx10^(-3) mol dm^(-3) atm^(-1)

Calculate the entropy change in surroundings when 1.0 mol of H_2O (l) is formed under standard conditions. Given Delta_fH^@ = -286 kJ mol^-1

The statement " if 0.003 moles of a gas are dissolved in 900 g of water under a pressure of 1 atmosphere , 0.006 moles will be dissolved under a pressure of 2 atmospheres ". Illustrates : ____.