1. Determine the partial pressure of hydrogen gas 2. Determine the amount of hyd

Question

1. Determine the partial pressure of hydrogen gas

2. Determine the amount of hydrogen gas (in moles) produced from the magnesium metal.

3. Use the Combined Gas Law to determine the experimental volume of hydrogen gas at STP.

4. Determine the experimental molar volume of hydrogen gas at STP conditions.

NAME SECTION DATE DATA SHEET (1I) Mass of Magnesium (2) Volume of hydrogen gas mL (3)Temperature of hydrogen gas (4) Atmospheric pressure °c mmHg (5) Vapor pressure of water (Table 1)mmHg ATIONS ine the partial pressure of hydrogen gas.

Explanation / Answer

Q1.

pressure of gas -->

Pgas = Ptotal - Pvapor = 764.54-20 = 744.54 mm Hg

Q2

find moles of H2(g)

PV = nRT

n = PV/(RT) = (744.54 *47.2*10^-3)/(0.082*(22+273))

n = 1.45276

1 mol of MG = 1 mol of H2

1.45276 mol of Mg reacted

c)

At STP

1 mol of gas = 22.4 L

1.45276 mol of gas --> 1.45276*22.4 = 32.541 L of gas

Hydrogen at STP -- >22. 4L so this is pretty near

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