Equal masses of `SO_(2)` and `O_(2)` are kept in a vessel at `27^(@)C`.The total pressure of the mixture is 2.1 atm.The partial pressure of `SO_(2)` ,is
1.4 atm
7 atm
0.7 atm
14 atm

Equal mass of H_(2) , He and CH_(4) are mixed in empty container at 300 K, when total pressure is 2.6 atm The partial pressure of H_(2) in the mixture is

In a mixture of N_2 and CO_2 gases, the partial pressure of CO_(2) is 1.25 atm. The total pressure of the mixture is 5 atm. The mole fraction of N_(2) in the mixture is

N_(2)O_(3) dissociates into NO and NO_(2) . At equilibrium pressure of 3 atm , all three gases were found to have equal number of moles in a vessel. In another vessel, equimolormixture of N_(2)O_(3), NO and NO_(2) are taken at the same temperature but at an initial pressure of 9 atm then find the partial pressure of NO_(2) (in atm ) at equilibrium in second vessel! N_(2)O_(3)(g) hArr NO(g) + NO_(2) (g)

If 1 mole of H_(2) , 2 moles of O_(2) and 3 moles of N_(2) are mixed in a vessel and total pressure was found to be 12 atm then the partial pressure exerted by N_(2) in the vessel will be

At 27^(@)C and 7.0 atm pressure, the density of propene gas is :

60 g of gaseous C_(2)H_(6) are mixed with 28 g of carbon monoxide. The pressure of the resulting gaseous mixture is 3 atm. The partial pressure in atm. Of C_(2)H_(6) in the mixture is

At 27^(@)C and 2.0 atm pressure, the density of propene gas is :

At 27^(@)C and 4.0 atm pressure, the density of propene gas is :

When NO and NO_(2) are mixed, the following equilibria are readily obtained, 2NO_(2) hArr N_(2)O_(4), K_(p)=6.8 atm^(-1) NO+NO_(2) hArr N_(2)O_(3) In an experiment when NO and NO_(2) are mixed in the ratio of 1:2 , the final total pressure was 5.05 atm and the partial pressure of N_(2)O_(4) was 1.7 atm. Calculate a. the equilibrium partial pressure of NO . b. K_(p) for NO+NO_(2) hArr N_(2)O_(3) .

If 200mL of He at 0.66 atm and 400 mL of O_(2) at 0.52 atm pressure are raised in 400 mL vessel at 20^(@)C then find the partial pressures of He and O_(2) ?