Asked by Jess
What amount of hydrogen peroxide should result when 1.21 g of barium peroxide is treated with 25.1 mL of hydrochloric acid solution containing 0.0289 g of HCl per mL?
Answers
Answered by
DrBob222
1. Write the equation and balance it.
2a. Convert 1.21 g BaO2 to moles. mol = grams/molar mass.
2b. Do the same for the HCl. 0.0289 g/mL x 25.1 mL = grams, then mols = g/molar mass
3a. Using the coefficients in the balanced equation, convert mols BaO2 to moles of the product.
3b. Same for HCl
3c. You get two answers and only one can be right. The correct answer in limiting reagent problems is ALWAYS the smaller one and the reagent producing that value is the limiting reagent.
4. Using the smaller value, convert that to g. g = mols x molar mass.
2a. Convert 1.21 g BaO2 to moles. mol = grams/molar mass.
2b. Do the same for the HCl. 0.0289 g/mL x 25.1 mL = grams, then mols = g/molar mass
3a. Using the coefficients in the balanced equation, convert mols BaO2 to moles of the product.
3b. Same for HCl
3c. You get two answers and only one can be right. The correct answer in limiting reagent problems is ALWAYS the smaller one and the reagent producing that value is the limiting reagent.
4. Using the smaller value, convert that to g. g = mols x molar mass.
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.