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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

the enthalpy of formation of water is given as -285.8kj/mol, which states that the enthalpy of formation is negative.

negative enthalpy of formation indicates that the heat is released during the reaction process. the heat is released from reaction to the surroundings the enthalpy is expressed with a negative sign with the energy given out in the reaction process.

the formation of water takes place by giving out heat which is -285.8 kj/mol.

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