The combustion of ethanol, C2H6O (MW = 46.0 g/mol), produces CO2 (MW = 44.0 g/mol) and water (18.0 g/mol). In a lab experiment, the reaction occurs using 4.60 g of ethanol in a 1.00 L container at body temperature (310 K) and 0.970 atm according to the following equation:
2C2H6O(l) + 7O2 (g) -> 4CO2 (g) + 6H2O (g)
What is the partial pressure of CO2?
What sequence of the following steps should you use to solve the problem using the KNU method?
A: Plug the numeric result of the determination of (#mol(ETOH)) in the expression of the n(CO2)
B: Figure out the expression of (#mol(EtOH)) using the relation between (#mol(EtOH)), the weight (wt) and the molar weight (MW) of EtOH in the form (#mol(EtOH)) = ...
C: Plug the numeric result of the determination of n(CO2) in the expression of the requested pressure of CO2
D: Set up the expression of the requested answer using the relation between the pressure of CO2 (P(CO2)), number of moles of CO2 (n(CO2)), the temperature (T) and the volume (V) of the reaction container in the form
P(CO2)) = ...
E: Figure out the expression of n(CO2) using the relation between n(CO2) and the number of moles of ethanol (#mol(EtOH)) by way of the mole ratio of CO2/EtOH in the from n(H2O) =