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What will be the pressure of the gas mixture when 0.5 l of h2 at 0.8 bar and 2 l of o2 at 0.7 bar are introduced in a 1 l vessel at 27℃? What will be the pressure of the gas mixture when 0.5 l of h2 at 0.8 bar and 2 l of o2 at 0.7 bar are introduced in a 1 l vessel at 27℃?
Use gaseous formula , PV = nRT => n = PV/RTnow, moles of H2 = PV/RT for H2, pressure ( P ) = 0.8 bar and volume ( V ) = 0.5 L ,moles of H2 = 0.8 × 0.5/RT = 0.4/RTsimilarly for O2, pressure ( P ) = 0.7 bar , volume ( V ) = 2 Lmoles of O2 = PV/RT = 0.7 × 2/RT = 1.4/RT hence, total number of moles = 0.4/RT + 1.4/RT = 1.8/RT now, Total pressure = n'RT/V' [ by gas formula]here, n' is Total moles = 1.8/RT V' is total volume = 1 Lnow, total pressure = 1.8/RT × RT/1 = 1.8 atm
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