Question

reaction stoichiometry involving gases 79. consider the chemical reaction: c(s) + h₂o(g) ⟶ co(g) + h₂(g) how many liters of hydrogen gas are formed from the complete reaction of 22.5 g c? assume that the hydrogen gas is collected at a pressure of 1.00 atm and a temperature of 355 k. missed this? read section 6.7; watch iwe 6.12

Explanation:

Step1: Calculate moles of C

Molar mass of C is 12.01 g/mol. Moles of C = $\frac{22.5\ g}{12.01\ g/mol} \approx 1.874\ mol$.

Step2: Relate moles of C to H₂

From the reaction $C(s) + H_2O(g)
ightarrow CO(g) + H_2(g)$, 1 mol C produces 1 mol H₂. So moles of H₂ = 1.874 mol.

Step3: Use ideal gas law (PV = nRT)

R = 0.0821 L·atm/(mol·K), P = 1.00 atm, T = 355 K, n = 1.874 mol.
Rearrange for V: $V = \frac{nRT}{P} = \frac{1.874\ mol \times 0.0821\ L·atm/(mol·K) \times 355\ K}{1.00\ atm}$.
Calculate: $V \approx \frac{1.874 \times 0.0821 \times 355}{1} \approx 54.0\ L$.

Answer:

Approximately 54.0 liters.