In a closed container nitrogen and hydrogen mixture initially ina a mole ratio of `1:4` reached equilibrium. It is found that the half hydrogen is converted to ammonia. If the original pressure was 180 atm, what will be the partial pressure of ammonia at equilibrium. (There is no change in temperature).

A cylinder contains 0.3 moles of N_(2) , 0.1 mole of O_(2) and 0.1 mole of helium. If the total pressure is one atm, what is the partial pressure of oxygen in mm Hg:-

The masspercentage in composition of dry air at sea level contains contains approximately 75.5% of N_(2) . If the total atmosphere pressure is 1 atm then what will be the partial pressure of nitrogen? [Given : average molecular mass of air = 29 ]

Final pressure is higher than initial pressure of a container filled with an ideal gas at constant temperature. What will be the value of equilibrium constant ?

Consider one mole of perfect gas in a cylinder of unit cross section with a piston attached as shown in figure. A spring (spring constant k) is attached (unstretched length L ) to the piston and to the bottom of the cylinder. Initially the spring is unstretched and the gas is in equilibrium. A certain amount of heat Q is supplied to the gas causing an increase of value from V_0 to V_1 . (a) What is the initial pressure of the system ? (b) What is the final pressure of the system ? (c) Using the first law of thermodynamics, write down a relation between Q, P_a , V, V_0 and k.

A container of fixed volume has a mixture of a one mole of hydrogen and one mole of helium in equilibrium at temperature T. Assuming the gasses are ideal, the correct statement (s) is (are)

Two cylinders A and B of equal capacity are connected to each other via a stopcock. A contains a gas at standard temperature and pressure. B is completely evacuated. The entire system is thermally insulated. The stopcock is suddenly opened. Answer the following: (a) What is the final pressure of the gas in A and B ? (b) What is the change in internal energy of the gas ? (c) What is the change in the temperature of the gas ? (d) Do the intermediate states of the system (before settling to the final equilibrium state) lie on its P-V-T surface ?

In the equilibrium H_(2)+I_(2)hArr2HI the number of moles of H_(2),I_(2) and HI are 1,2,3 moles respectively. Total pressure of the reaction mixture is 60 atm. Calculate the partial pressures of H_(2),I_(2) and HI in the mixture.