The density of a mixture of `CH_(4)` and `SO_(2)`gases at NTP is 1.25g/litre .Calculate partial pressure in atm of `CH_(4)`. Report your answer after multiplying it by 100.

If the density of a mixture of O_(2)&N_(2) at N.T.P. is 1.258 g//l. The partial volume of O_(2) in 3 mole of mixture is

The density of a mixturee of O_(2) and N_(2) gases at 1 atm and 273 K is 0.0013 gm/mL. If partial pressure of O_(2) in the mixture is A, then calculate value of 25 A.

The total pressure of a gaseous mixture of 2.8 g N_(2) , 3.2 g O_(2) , and 0.5 g H_(2) is 4.5 atm . Calculate the partial pressure of each gas.

If osmotic pressure of 1M aqueous solution of H_(2)SO_(4) at 500K is 90.2 atm. Calculate K_(a2) of H_(2)SO_(4) . Give your answer after multiplying 1000 with K_(a2) . (Assuming ideal solution). (Given: K_(a1) of H_(2)SO_(4) is oo,R=0.082 l t-atm//mol-K) .

The vapour density of the mixture at equilibrium is 38.3 at 33^(@)C N_(2)O_(4) (g) hArr 2NO_(2) (g) Determine the value of degree of dissociation. Report your answer the multiplying by 10 .

At 25^(@)C and 1 atm pressure, the partial pressure in equilibrium mixture of N_(2)O_(4) and NO_(2) , are 0.7 and 0.3 atm , respectively. Calculate the partial pressures of these gases when they are in equilibrium at 25^(@)C and a total pressure of 10 atm .