What is the mass of #CO2# formed when 1.00kJ of energy is released? Full question in the description box below as an image.

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1 Answer
Jan 10, 2018

The mass of #"CO"_2# formed is 129 mg.

Explanation:

Step 1. Write the balanced equation for the reaction

#"C"_2"H"_5"OH" + "3O"_2 → "2CO"_2 + "3H"_2"O"; Δ_text(c)H = "-1366.3 kJ·mol"^"-1"#

Step 2. Calculate the moles of #"CO"_2# formed

#n_text(CO₂) = 1.00 color(red)(cancel(color(black)("kJ"))) × (1 color(red)(cancel(color(black)("mol C"_2"H"_5"OH"))))/(1366.3 color(red)(cancel(color(black)("kJ"))))× ("2 mol CO"_2)/(1 color(red)(cancel(color(black)("mol C"_2"H"_5"OH")))) = "0.001 464 mol CO"_2#

Step 3. Calculate the mass of #"CO"_2# formed

#m_text(CO₂) = "0.001 464" color(red)(cancel(color(black)("mol CO"_2))) × "44.01 g CO"_2/(1 color(red)(cancel(color(black)("mol CO"_2)))) = "0.0644 g CO"_2 = "64.4 mg CO"_2#