Asked by Tasha
Based on the following chemical equation, answer the questions below. Show all your calculation
The balanced chemical reaction of iodine with hydrogen sulfide is as follows:
H2S(g)+I2(s)-----2HI(g) + S(s)
(a) Based on the above chemically balanced equation, how many grams of HI should be produced from the reaction of 25.0g of H2S when there is excess amount of I2?
(b) Actually 30.0g of HI is produced in this reaction, what is the percent yield of HI?
The balanced chemical reaction of iodine with hydrogen sulfide is as follows:
H2S(g)+I2(s)-----2HI(g) + S(s)
(a) Based on the above chemically balanced equation, how many grams of HI should be produced from the reaction of 25.0g of H2S when there is excess amount of I2?
(b) Actually 30.0g of HI is produced in this reaction, what is the percent yield of HI?
Answers
Answered by
DrBob222
a. mols H2S = grams/molar mass
Use the coefficients in the balanced equation to convert mols H2S to mols HI. That will be ?mols H2S x (2 mols HI/1 mol H2S) = ?mols H2S x 2/1 = ? mols HI
Then convert mols HI to grams HI. grams = mols x molar mass. This is the theoretical yield (TY).
b. Actual yield (AY) is 30.0 g.
%yield = (AY/TY)*100 = ?
Use the coefficients in the balanced equation to convert mols H2S to mols HI. That will be ?mols H2S x (2 mols HI/1 mol H2S) = ?mols H2S x 2/1 = ? mols HI
Then convert mols HI to grams HI. grams = mols x molar mass. This is the theoretical yield (TY).
b. Actual yield (AY) is 30.0 g.
%yield = (AY/TY)*100 = ?
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.