PROBLEM 91P

CH3OH can be synthesized by the reaction:

CO(g) + 2H2(g) → CH3OH(g)

How many liters of H2 gas, measured at 748 mm Hg and 86 °C, are required to synthesize 0.55 mol of CH3OH? How many liters of CO gas, measured under the same conditions, are required?

Solution 91P

CH3OH can be synthesized by the reaction:

CO(g) + 2H2(g) → CH3OH(g)

Given that

Temperature =86 oC.

Given moles =0.55 mol of CH3OH.

Equations and conversion factors used

1 mole of CH3OH=2 mol of H2.

No .of moles of H2 required to synthesis 0.55 mol of CH3OH= 0.55 mol of CH3OH *2 mol of H2/1 mol of CH3OH.

The similar will get cancel.the result is 1.1 mol of H2.

PV=nRT

Pressure = 748 mm of Hg

Temperature =860C.

n=1.1 moles of H2

R=8.314 J

According to the formula the calculations are given below

V=nRT/P

=1.1 *8.314*86/748 mm of Hg

=1.0514 volume of CO requried.