What will be the pressure of the gaseous mixture when 0.5 L of `H_2` at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1 L vessel at `27^@C`?

Explanation

Case -I Hydrogen gas
` P_1 = 0.8 ` bar
` P_2 =?`
` V_1 = 0.5 lit`
` V_2 = 1.0 lit `
` P_1 V_1 = P_2 V_2`
` P_2 = (0.8 xx 0.5)/(1) `
` P_2 = 0.4` bar
Partial pressure of `H_2 = 0.4 `bar. [`P_(H_2)`]
Case -II
oxygen gas
` P_1= 0.7 ` bar
` V_1 = 2 lit`
` V_2 = 2 lit `
`P_2 =?`
`P_1 V_1 = P_2 V_2`
` P_2 = (P_1 V_1)/(V_2 ) = ( 0.7 xx 2 )/(1) `
`= 1.4` bar
Partial pressure of `O_2 = 1.4 `bar. [`p_(O_2)`]
` therefore ` Total pressure = ` P_(H_2) +P_(O_2)`
` = 0.4 +1.4 = 1.8 ` bar