We can start by using the given enthalpy change and the balanced equation to calculate the amount of moles of carbon dioxide produced:
1 mol of C2H5OH produces 2 mol of CO2
-1367 kJ/mol is released when 1 mol of C2H5OH is combusted
370 kJ of energy are used in the reaction
Now we can use a proportion to find the number of moles of C2H5OH that produce 370 kJ of energy:
-1367 kJ/mol / 1 mol of C2H5OH = -x kJ / (2 mol of CO2)
Solving for x gives:
x = (370 kJ) (1 mol of C2H5OH) / (-1367 kJ/mol) (2 mol of CO2)
x = 0.1355 mol of CO2
Finally, we can use the molar mass of CO2 (44.01 g/mol) to find the mass of CO2 produced:
mass of CO2 = number of moles of CO2 * molar mass of CO2
mass of CO2 = 0.1355 mol * 44.01 g/mol = 5.96 g of CO2
Therefore, when 370 kJ of energy are used in the reaction, 5.96 g of carbon dioxide are produced.