Question

Carbon monoxide reacts with oxygen to form carbon dioxide by the following reaction: 2 CO(g) + O2(g) → 2 CO2(g) ∆H for this reaction is −135.28 kcal. How much heat would be released if 12.0 moles of carbon monoxide reacted with sufficient oxygen to produce carbon dioxide?

Answer 1

Answer:

$\large \boxed{\text{811.68 kcal}}$

Explanation:

It is often convenient to treat the heat of reaction as if it were a reactant or a product. For this reaction, we could write

2CO + O₂ ⟶ 2CO₂ + 135.28 kcal

We could consider the “kcal” as an element with 135.28 as the coefficient in the equation.

The molar ratio would be 135.28 kcal:2 mol CO . Then,

$\text{Heat released} = \text{12.0 mol CO} \times \dfrac{\text{135.28 kcal}}{\text{2 mol CO}} = \textbf{811.68 kcal}\\\\\text{The reaction releases \large \boxed{\textbf{811.68 kcal}} }$

Answer 2

Answer:

Heat released =811.68kcal

Explanation:

2 CO(g) + O2(g) → 2 CO2(g)                 ΔH=-135.28kcal

for this type of question 1st balance the chemical reaction and use unitry method.

From the above balanced equaion it is clearly that,

2 mole of CO reacts with 1 mole of O2 and we have sufficient amount of oxygen means excess amount.

and also for complete consumption of 2 mole of CO, ΔH=-135.28 kcal

for complete consumption of 12 moles of CO2 ΔH=$6\times (-135.28kcal)$

Heat released =811.68kcal