Vapor pressure of water at 20 oC = 17.5 mmHg
Partial pressure of H2 gas = (Atmospheric pressure) - (Vapor pressure of water at 20 oC)
Partial pressure of H2 gas = (760 mmHg) - (17.5 mmHg)
Partial pressure of H2 gas = 742.5 mmHg
Partial pressure of H2 gas = 742.5 mmHg * (1 atm / 760 mmHg)
Partial pressure of H2 gas = 0.977 atm
(a) Using ideal gas law PV = nRT
n = PV / RT
moles H2 produced = [(pressure H2) * (volume H2)] / [(R) * (Temperature H2)]
where volume H2 = 8 mL = 8 x 10-3 L
R = gas constant = 0.0821 L-atm/mol-K
Temperature H2 = 20 oC = 293 K
Substituting the values,
moles H2 produced = [(0.977 atm) * (8 x 10-3 L)] / [(0.0821 L-atm/mol-K) * (293 K)]
moles H2 produced = 3.25 x 10-4 mol
(b) moles X = (moles H2 produced) * (1 mole X / 1 mole H2)
moles X = (3.25 x 10-4 mol) * (1 / 1)
moles X = 3.25 x 10-4 mol
(c) molar mass of metal = (mass of metal) / (moles of metal)
molar mass of metal = (0.29 g) / (3.25 x 10-4 mol)
molar mass of metal = 892.5 g/mol
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