Question

À chemist reacted 17.25 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is showr
Na + ch2- Nacl
If the percentage yield of the reaction is 88%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors.

Answer 1

Answer:

Actual yield is 38.57

Explanation:

Percentage yield = Actual yield / theoretical yield X 100

Percent yield x theoretical yield / 100 = actual yield

Write the balanced chemical equation:

2Na + CI2 = 2NaCI

Given is 17.25 g Sodium metal (limiting reactant) with excess being chlorine gas

Percent yield is 88%

Mole of Na = 17.25 g / 22.98 = 0.750

Calculate the Theoretical Yield to solve for Actual Yield

Theoretical yield = 0.75 x molar mass of NaCI

Theoretical yield = 0.75 x 58.44 = 43.83 g

When plugged into the original percentage yield formula:

Actual yield = 88 x 43.83 / 100 = 38.57 g