How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below?

Question

Chemistry

Lucas Rodgers

3 December, 10:16

How many grams of water are required to produce 5.50 L of hydrogen gas at 25.0°C and 755 mm Hg pressure according to the chemical equation shown below?

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Nibby · Answer 1

Answer is: 4.02 grams of water are required.

Chemical reaction: BaH₂ + 2H₂O → Ba (OH) ₂ + 2H₂.

Ideal gas law: p·V = n·R·T.

p = 755 mm Hg : 760.0 mmHg / atm = 0.993 atm.

T = 25 + 273.15 = 298.15 K.

V (H ₂) = 5.50 L.

R = 0,08206 L·atm/mol·K.

n (H ₂) = 0.993 atm · 5.5 L : 0,08206 L·atm/mol·K · 298.15 K.

n (H ₂) = 0.223 mol.

From chemical reaction: n (H ₂O) : n (H₂) = 1 : 1.

n (H₂O) = 0.223 mol.

m (H₂O) = 0.223 mol · 18 g/mol.

m (H₂O) = 4.02 g.