# The fuel methanol (CH_3OH) is made by the reaction of carbon monoxide and hydrogen. What is the balanced chemical equation? How many grams of hydrogen are needed to produce 45.0 grams of methanol?

Mar 26, 2016

The balanced equation is: $2 {H}_{2} + C O \to C {H}_{3} O H$. It requires 2 moles of ${H}_{2}$ to make each mole of $C {H}_{3} O H$, for a total of $5.64$ $g$ required. (See the full calculation below.)

#### Explanation:

The balanced equation is: $2 {H}_{2} + C O \to C {H}_{3} O H$.

One C, one O and 4 H on each side.

The molar mass of methanol is $12 + 4 + 16 = 32$ $g m o {l}^{-} 1$

Number of moles: $n = \frac{m}{M} = \frac{45}{32} = 1.41$ $m o l$

From the balanced equation we know that it takes 2 moles of ${H}_{2}$ to produce each mole of methanol, so we need $2.82$ $m o l$ of ${H}_{2}$.

To find the mass, $m = n M = 2.82 \cdot 2 = 5.64$ $g$ of ${H}_{2}$.