From the \"Determination of the Molar Volume of a Gas and the Gas Constant, R\"

Question

From the "Determination of the Molar Volume of a Gas and the Gas Constant, R" Lab: (HCl, Magnesium Ribbon, Copper wire,etc. is used in the lab) 1. A student did the experiment described except she used Al foil instead of Mg. Her data table included the following values: Mass of Al - 0.0352 grams Temperature - 19.08 celsius Barometric Pressure - 762.5 mmHg Volume of H2 Gas - 46.92 mL Answer the following questions based on this data table.

1e. What was the pressure of the dry hydrogen?

1f. Determine the experimental value of the gas constant, R.

1g. Determine the volume of the dry H2 gas at STP conditions.

1h. Determine the experimental value of volume of dry H2 gas at STP per mole of H2.

1i. Why is there a lag time in this experiment between the inverting of the eudiometer tube and the start of the reaction between the metal and HCl?

Explanation / Answer

(e)

Vapour pressure of dry H2 gas = 762.5 - 23.75 = 738.75 mmHg = 738.75 / 760 = 0.972 atm

(f)

Ideal gas equation,

P V = n R T

0.972 * 0.04692 = 0.00196 * R * 273.15

R = 0.0852 L.atm.K-1.mol-1

(g)

At STP,

P = 1.00 atm and T = 273.15

1.00 * V = 0.00196 * 0.0852 * 273.15

V = 0.0456 L

(h)

Volume of dry H2 per mol = V / n = 0.0456 / 0.00196 = 23.3 L

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