Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. What is the theoretical yield of carbon dioxide formed from the reaction of 18.0g of ethane and 57.8g of oxygen gas?

46.97g

Explanation:

Hello,

To find the theoretical yield, we must first of all get the equation of reaction right in order to know how the compounds combine together.

Equation of reaction;

2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O

From the equation of reaction,

2 moles of C₂H₆ reacts with 7 moles of O₂ to produce 4 moles of CO₂.

Number of moles = mass / molar mass

Mass = number of moles × molar mass

Mass of CO₂ = 4 × 44 = 176g

Mass of C₂H₆ = 2 × 30 = 60g

Mass of O₂ = 7 × 32 = 224g

Therefore, 224g + 60g (O₂ + C₂H₆) = 176g of CO₂.

284g of reactants = 176g of product(CO₂)

(18 + 57.8)g of reactants = x g of products(CO₂)

X = (75.8 × 176) /284

X = 46.97g of CO₂.

Theoretical yield of CO₂ is 46.97g

altitude, density, pressure

air gets less dense the higher the altitude and also the air pressure is less as altitude rises.

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.