How many grams of water are required to produce 5.50L of hydrogen gas at 25.0 degrees C and 755mmHg?

Question

Chemistry

Linda Trevino

16 August, 10:34

How many grams of water are required to produce 5.50L of hydrogen gas at 25.0 degrees C and 755mmHg?

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Answers (1)

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Zain Ochoa · 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 (H₂) = 5.50 L.

R = 0,08206 L·atm/mol·K.

n (H₂) = 0.993 atm · 5.5 L : 0,08206 L·atm/mol·K · 298.15 K.

n (H₂) = 0.223 mol.

From chemical reaction: n (H₂O) : n (H₂) = 1 : 1.

n (H₂O) = 0.223 mol.

m (H₂O) = 0.223 mol · 18 g/mol.

m (H₂O) = 4.02 g.