Question

1. carbon dioxide gas and hydrogen gas react to form methanol gas and water. assuming the process is 100 percent efficient and at stp, how many liters of each reactant are needed to obtain 0. 700 l of methanol? the reaction is : \\(\ce{co_{2}(g) + 3h_{2}(g) \

ightarrow ch_{3}oh(g) + h_{2}o(g)}.\\) \
solution:\
\
a.\
\
\
\
b.

Explanation:

Step1: Relate CO₂ to CH₃OH via mole ratio

At STP, gas volume ratio = mole ratio. From the reaction, 1 mole $\text{CO}_2$ produces 1 mole $\text{CH}_3\text{OH}$.
$\text{Volume of CO}_2 = \text{Volume of CH}_3\text{OH} \times \frac{1\ \text{mol CO}_2}{1\ \text{mol CH}_3\text{OH}}$
$\text{Volume of CO}_2 = 0.700\ \text{L} \times \frac{1}{1} = 0.700\ \text{L}$

Step2: Relate H₂ to CH₃OH via mole ratio

From the reaction, 3 moles $\text{H}_2$ produce 1 mole $\text{CH}_3\text{OH}$.
$\text{Volume of H}_2 = \text{Volume of CH}_3\text{OH} \times \frac{3\ \text{mol H}_2}{1\ \text{mol CH}_3\text{OH}}$
$\text{Volume of H}_2 = 0.700\ \text{L} \times \frac{3}{1} = 2.10\ \text{L}$

Answer:

Volume of $\text{CO}_2$ needed: $0.700\ \text{L}$
Volume of $\text{H}_2$ needed: $2.10\ \text{L}$