When 37.1 g of CH4 reacts completely with excess chlorine yielding 52.0 g of HCl, what is the percentage yield, according to CH4 (g) + Cl2 (g) → CH3Cl (g) + HCl (g) Group of answer choices

Percent yield = 63.7%

Explanation:

Given dа ta:

Mass of CH₄ = 37.1 g

Actual yield of HCl = 52.0 g

Percent yield = ?

Solution:

Chemical equation:

CH₄ + Cl₂ → CH₃Cl + HCl

Number of moles of CH₄:

Number of moles = mass / molar mass

Number of moles = 37.1 g / 16 g/mol

Number of moles = 2.3 mol

Now we compare the moles of HCl with CH₄.

CH₄ : HCl

1 : 1

2.3 : 2.3

Theoretical yield:

Mass of HCl = number of moles * molar mass

Mass of HCl = 2.3 mol * 35.5 g/mol

Mass of HCl = 81.65 g

Percent yield:

Percent yield = Actual yield / theoretical yield * 100

Percent yield = 52.0 g / 81.65 g * 100

Percent yield = 63.7%