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8.60 moles of Carbon monoxide combine with Hydrogen to produce Methanol. Determine:

Liters of Hydrogen needed

= 385.28L

Explanation:

Molecular mass of CO = (12+16) = 28g

Molecular mass of CH3OH = (28+4) = 32g

Molecular mass of H2 = (1+1) = 2g

CO(g) + 2H2(g) > CH3OH(l)

moles: 1. 2. 1

1 mole of CO reacts with 2 moles of H2

8.6moles of CO will react with ( 8.6 × 2 )

= 17.2 moles of Hydrogen.

At Standard Temp and Pressure ( s.t.p )

1 mole of H2 occupies 22.4L

17.2 moles of H2 will occupy ( 22.4 × 17.2 )

= 385.28L