The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ)released to the surroundings when 10.0 g of CO (g)reacts completely. 2CO (g) + O₂ (g) → 2CO₂ (g) A)2410 kJ B)172 kJ C)86.0 kJ D)482 kJ E)-482 kJ

Question

Quizplus · Accepted Answer

1. Write the balanced chemical equation:
2CO (g) + O2 (g) → 2CO2 (g)

2. Calculate the moles of CO used in the reaction:
10.0 g CO / 28.01 g/mol = 0.356 mol CO

3. Use the balanced chemical equation to determine the moles of O2 used and CO2 produced:
2 mol CO : 1 mol O2 : 2 mol CO2
0.356 mol CO × (1 mol O2 / 2 mol CO) = 0.178 mol O2
0.356 mol CO × (2 mol CO2 / 2 mol CO) = 0.356 mol CO2

4. Calculate the heat released using the equation: 
q = ΔH° × n = -482 kJ/mol × 0.356 mol CO = -171.8 kJ ≈ -172 kJ (rounded to three significant figures)

5. The negative sign in the answer indicates that the reaction is exothermic (releases energy to the surroundings).

The Value of ΔH° for the Reaction Below Is -482