Question

Chemistry question help fast?

1) Given the following reaction:

4 KO2 + 2 H2O + 4 CO2 --> 4 KHCO3 + 3 O2

How many moles of O2 will be produced if 5.75 moles of CO2 react completely?

2) A chemical reaction occurs between solutions of KCl and silver nitrate. This reaction produces a precipitate that is recovered, dried and massed. The mass of the precipitate is found to be 11.438650. What is the percent yield of the reaction if 72.3135 grams of KCl was reacted with excess silver nitrate?

Answers

1)

4 KO2 + 2 H2O + 4 CO2 → 4 KHCO3 + 3 O2

(5.75 mol CO2) x (3/4) = 4.31 mol O2

2)

KCl + AgNO3 → AgCl + KNO3

(72.3135 g KCl) / (74.5515 g/mol) x (1/1) x (143.3214 g/mol) = 139.019 g AgCl in theory

11.438650 g / 139.019 g = 8.228%

(That's an exceptionally poor yield for that kind of reaction. Are you sure you place the decimal point correctly in "11.438650"?)

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