A. You have the balanced equation.
1. Convert 8.87 g As2O3 to mols remembering that mols = grams/molar mass.
2. Using the coefficients in the balanced equation, convert mols As203 to mols As.
3. Convert mols As to grams. grams = mols x molar mass. This is the theoretical yield.
4. %yield =
(actual yield/theoretical yield)x 100
B. The procedure is the same for this part of the problem but you start with carbon. Post your work if you get stuck.
In the commercial production of the element arsenic, arsenic (II) oxide is heated with carbon which reduces the oxide to the metal according to the following equation: 2As2O3 + 3C ----„³ 3CO2 +4As
A>if 8.87 g of As2O3 is used in the reaction and 5.33 g of As is produced what is the percentage yield?
B>If 67 of carbon is used up in a different reaction and 425 g of As is produced, calculate the percentage yield of this reaction
2 answers
79.3%
1 answer