Question

2 co(g) + c(g) → c₃o₂(g) δh° = 127.3 kj/molᵣₓₙ
the equation shown above represents an endothermic reaction between co(g) and c(g). what is the amount of heat absorbed when 1.00 mol of co(g) reacts with an excess of c(g) ?
a 31.8 kj
b 63.7 kj
c 127.3 kj
d 254.6 kj

Explanation:

Step1: Analyze the reaction stoichiometry

The given reaction is \( 2\ \text{CO}(g) + \text{C}(g)
ightarrow \text{C}_3\text{O}_2(g) \) with \( \Delta H^{\circ} = 127.3\ \text{kJ/mol}_{\text{rxn}} \). This means that when 2 moles of \( \text{CO}(g) \) react, 127.3 kJ of heat is absorbed.

Step2: Calculate heat for 1 mole of CO

We need to find the heat absorbed for 1 mole of \( \text{CO}(g) \). Let \( x \) be the heat absorbed for 1 mole of \( \text{CO}(g) \). Using the ratio of moles of \( \text{CO} \) to heat absorbed:
\[
\frac{2\ \text{mol CO}}{127.3\ \text{kJ}} = \frac{1\ \text{mol CO}}{x}
\]
Solving for \( x \):
\[
x = \frac{127.3\ \text{kJ} \times 1\ \text{mol CO}}{2\ \text{mol CO}} = 63.65\ \text{kJ} \approx 63.7\ \text{kJ}
\]

Answer:

B. 63.7 kJ