Question

CH3OH can be synthesized by the following reaction.
CO(g)+2H2(g)→CH3OH(g)

What volume of H2 gas (in L), measured at 746 mmHg and 84 ∘C, is required to synthesize 23.4 g CH3OH?

How many liters of CO gas, measured under the same conditions, is required?

Answer 1

Number of moles of CH3OH = 23.4 g / 32.04 g/mol = 0.730 mole

From the balanced equation we can say that

1 mole of CH3OH requires 2 mole of H2 so

0.730 mole of CH3OH will require

= 0.730 mole of CH3OH *(2 mole of H2 / 1 mole of CH3OH)

= 1.46 mole of H2

PV = nRT

P = 746 mmHg = 0.982 atm

V = ?

T = 84 + 273 = 357 K

0.982 * V = 1.46 * 0.0821 * 357

0.982 *V = 42.8

V = 42.8 / 0.982 = 43.6 L

Therefore, volume of H2 gas required would be 43.6 L

From the balanced equation we can say that

1 mole of CH3OH requires 1 mole of CO so

0.730 mole of CH3OH will require 0.730 mole of CO

PV = nRT

0.982 * V = 0.730 * 0.0821 * 357

0.982 * V = 21.4

V = 21.4 / 0.982 = 21.8 L

Therefore, the volume of CO required would be 21.8 L