Answer:
2.0 mol of oxygen are consumed.
Step-by-step explanation:
You know that you will need a balanced equation with masses, moles, and molar masses, so gather all the information in one place.
M_r: 28.0 44.0
CO + ½O₂ ⟶ CO₂ + 67.6 kcal
m/g: 112
<em>Step 1</em>. Convert grams of CO to moles of CO
1 mol CO = 28.0 g CO
Moles of CO = 112 × 1/28.0
<em>Step 2.</em> Convert moles of CO to moles of CO₂.
The molar ratio is 1 mol CO₂ to 1 mol CO
Moles of CO₂ = 4.000 × 1/1
Moles of CO₂ = 4.00 mol CO₂
Option A is <em>wrong</em>.
<em>Step 3.</em> Calculate the amount of heat generated.
q = ΔH
The conversion factor is 67.6 kcal/1 mol CO₂
q = 4.00 × 67.6
q = 270 kJ
Option B is <em>wrong</em>, because it gives the heat generated by 1 mol of CO.
<em>Step 4. </em>Calculate the moles of O₂ consumed
Moles of O₂ = 2.00 mol O₂
Option C is correct.
<em>Step 5.</em> Calculate the moles of CO₂ formed
Already done in Step 2.
Moles of CO₂ = 4.00 mol CO₂
Option D is <em>wrong.
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<em>Step 6</em>. Calculate the moles of O₂ produced
Already done in Step 4.
Moles of O₂ = 2.00 mol O₂
Option E is <em>wrong.
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