Question

D Question 38 When 38.4 g of CH4 reacts completely with excess chlorine yielding 45.0 g of CH3CI, what is the percenta yield, according to CH4 +Clip -- CH3Clip + HCl 1212 853 O 629 37.1 O 147 Question

Answer 1

The percent yield of the reaction is 37.25%.

The percent yield can be calculated by dividing the actual yield (in this case, 45.0 g of CH3Cl) by the theoretical yield (the amount of CH3Cl that would be formed if all of the CH4 reacted). To find the theoretical yield, we need to calculate the amount of CH3Cl that would be formed from the given amount of CH4. Using the balanced equation:

CH4 + Cl2 → CH3Cl + HCl

We can determine that 1 mole of CH4 reacts to form 1 mole of CH3Cl. We can convert the given mass of CH4 to moles using its molar mass:

38.4 g CH4 × (1 mol CH4 / 16.04 g CH4)

= 2.392 mol CH4

Since the stoichiometric ratio is 1:1, the theoretical yield of CH3Cl is also 2.392 mol. We can then convert the moles of CH3Cl to grams:

2.392 mol CH3Cl × (50.49 g CH3Cl / 1 mol CH3Cl)

= 120.65 g CH3Cl

Now we can calculate the percent yield:

Percent Yield = (Actual Yield / Theoretical Yield) × 100

Percent Yield = (45.0 g CH3Cl / 120.65 g CH3Cl) × 100 = 37.25%