Calculate the total pressure in a mixture of 16 g of oxygen and 4g of Hydrogen confined in a vessel of 1dm-3 at 27 degree celsius. (Molar mass of oxygen 32 Hydrogen 2 R=0.083bar dm3 K-1mol-1)
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Moles of oxygen = 16 g / (32 g/mol) = 0.5 mol
Moles of Hydrogen = 4 g / (2 g/mol) = 2 mol
Total moles of gaseous mixture (n) = 0.5 + 2 = 2.5 mol
P = nRT / V
= (2.5 × 0.083 × 300) / 1
= 62.25 bar
Total pressure of gaseous mixture is 62.25 bar
Moles of Hydrogen = 4 g / (2 g/mol) = 2 mol
Total moles of gaseous mixture (n) = 0.5 + 2 = 2.5 mol
P = nRT / V
= (2.5 × 0.083 × 300) / 1
= 62.25 bar
Total pressure of gaseous mixture is 62.25 bar
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