EXPERIMENT 16 NAME DATE DATA TABLE A. Molar Volume of Hydrogen Gas mass of magne

Question

EXPERIMENT 16 NAME DATE DATA TABLE A. Molar Volume of Hydrogen Gas mass of magnesium volume of hydrogen gas temperature of hydrogen gas 007 ml °C mm Hg , mm Hg mm Hg mL. atmospheric pressure (see barometer) mm Hg vapor pressure of water (se Table 161) IYmm Hg vapor pressure of water (see Table 16.1) partial pressure of hydrogen gas mm Hg- Correct the volume of hydrogen gas to STP for trial I (see Example Exercise 16.1). RECYCLE Chemical volume of hydrogen gas (STH) Show the calculation for the moles of hydrogen gas for trial 1 (see Example Exercise 16.1). mol moles of hydrogen gas Show the calculation for the molar volume of hydrogen gas at STP for trial 1 . mol

Explanation / Answer

Calculation of molar volume

mass of Mg = 0.07 g

moles Mg = 0.07 g/24305 g/mol

                 = 0.003 mol

moles Mg = moles H2 (n)

                 = 0.003 mol

Volume (V2) of H2 = 41 ml

                               = 0.041 L

Temperature (T2) of H2 = 20 oC + 273

                                       = 293 K

Vapor pressure of H2O at 20 oC = 17.5 mmHg

atmospheric pressure = 738 mmHg

partial pressure of H2 (P2) = 738 - 17.5

                                           = 720.5 mmHg/760 mmHg

                                           = 0.95 atm

Volume of H2 at STP(V1) = P2V2T1/T2P1

with P1,V1 and T1 are STP values.

V1 at STP = 0.95 x 0.041 x 273.15/1 x 293

                 = 0.0363 L

molar volume = volume/moles

                       = 0.0363 L/0.003 mol

                       = 12.10 L/mol

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