Question

CHEM HELP ASAP!! What mass of H2 would be needed to produce 208 kg of methanol?

Answer 1

So if we use the equation:

$CO+2H_{2}$ → $CH_{3}OH$

We can then determine the amount of $H_{2}$ needed to produce 208 kg of methanol.

So let's find out how many moles of methanol 208 kg is:

Methanol molar weight = 32.041g/mol

So then we can solve for moles of methanol:

$208kg*\frac{1,000g}{1kg} *\frac{1mol}{32.041g} =6,491.68mol$

So now that we have the amount of moles produced, we can use the molar ratio (from the balanced equation) of hydrogen and methanol. This ratio is 2:1 hydrogen:methanol.

Therefore, we can set up a proportion to solve for the moles of hydrogen needed:

$\frac{2}{1} =\frac{x}{6,491.68}$

$x=12,983.36mol$

So now that we have the number of moles of $H_{2}$ that are produced, we can then use the molar weight of hydrogen to solve for the mass that is needed:

$12,983.36mol*\frac{2.016g}{1mol} =26,174.45g_H_{2}$

Therefore, the amount of diatomic hydrogen ($H_{2}$) that is needed to produce 208kg of methanol is $2.62x10^{4}$g.