4.62 ml c2h5OH ( m = 46.07 g/mol and density = 0.789g/mol) is combusted in the presence of 15.55g of o2 and 3.72 g of h2o . determine the precentage yeild c2h5oh10 + 3o2 = 2co2 + 3h2o

Mass of C2H5OH = 1.25 g Mass of H2O = 11.6 g Mass percent of C2H5 OH = 1.25 × 100 / 1.25 + 11.6 = 125 / 12.86...

n(C2H5OH)=m/M=10/46 = 0.2174 molH= (-1366.8)*0.2174 = -297.14 kJAnswer: -297.14 kJ

The volume of ethanol in 750 ml of wine is: 750 x 0.12 = 90 mlDensity = mass/volumeMass = density x volumeMass of pure ethanol = 0.789 x 90 =...

21,91 mole

Hence the %abundance of the two isotopes are 20 80 %.

C2H4 + 3O2 ---> 2CO2 + 2 H2OFrom Appendix table∆H°f C2H4 = 52.3Kj/mol∆H°fCO2= -393.5Kj/mol∆H°f H2O(g) = -241.8Kj/mol∆H°rxn= ∆H°products - ∆H°reactants∆H°rxn = [2(-393.5)+2(-241.8)] - [52.3]∆H°rxn = -1322.9KJ/mol

The mass of ethanol is found according to the equation: m = ρ × V, where ρ – the density and V – the volume. Thus, m = 0.789 g/ml...

Solution: The amount of substance of Oxygen: n(O2) = 3 mol *25 mol/1 mol = 75 mol Answer: By the reaction 75 mol of oxygen are needed.

Two reactions can be classified as combustion reactions: CH4 + O2 → CO2 + 2H2O C2H6O + 3O2 → 2CO2 + 3H2O

1 gallon= 3.785 L for US or the imperial gallon 1 gallon= 4.54609 L V=15 gallons×3.785 = 56.775 L=56.775×〖10〗^3 ml m=ρ×V=0.789 g/ml×56.775×〖10〗^3 ml≅44.795〖×10〗^3 g=44.795〖×10〗^6 mg Answer Ethanol’s mass must be...