What volume of H2 gas (in L), measured at 750 mmHg and 90 ∘C, is required to synthesize 24.6 g CH3OH?
The balanced equation is
CO (g) + 2 H2 (g) ------ > CH3OH (g)
number of moles of CH3OH = 24.6 g / 32.04 g/mol = 0.768 mole
from the balanced equation we can say that
1 mole of CH3OH requires 2 mole of H2 so
0.768 mole of CH3OH will require
= 0.768 mole of CH3OH *(2 mole of H2 / 1 mole of CH3OH)
= 1.54 mole of H2
PV = nRT
P = 750 mmHg = 0.987 atm
T = 273 + 90 = 363 K
0.987 * V = 1.54 * 0.0821 * 363
0.987 * V = 45.9
V = 45.9 / 0.987 = 46.5 L
Therefore, the volume of H2 needed would be 46.5 L
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