Stoichiometry Practice
Stoichiometry Practice
Stoichiometry Practice
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<strong>Stoichiometry</strong> l<br />
Show all the calculation setups and solutions.<br />
1. Use the given to solve the following problems:<br />
Na3PO4 (s) + 3 AgNO3 (aq) → Ag3PO4(s) + 3 NaNO3 (aq)<br />
a) How many moles of AgNO3 would be required to react with 1.0 mol<br />
of Na3PO4?<br />
b) How many moles of NaNO3 can be produced from 0.30 mol of<br />
Na3PO4?<br />
c) How many grams of Ag3PO4 can be produced from 4.00 g of AgNO3?<br />
d) If you have 8.44 g of Na3PO4, how many grams of AgNO3 will be<br />
needed to complete the reaction?<br />
e) When 25.0 g of AgNO3 are reacted with excess Na3PO4, 17.7 g of<br />
Ag3PO4 are produced. What is the percentage yield of Ag3PO4?
2. Use the equation given to solve the following problems.<br />
2 KMnO4 (aq) + 16 HCl (aq) → 5 Cl2 (g) + 2 KCl (aq) + 2 MnCl2 (aq) + 8 H2O (l)<br />
a) How many moles of HCl are required to react with 45 g of KMnO4?<br />
b) b) How many Cl2 molecules will be produced using 5.0 mol of<br />
KMnO4?<br />
c) To produce 55.0 g of MnCl2, what mass of HCl will be needed?<br />
d) How many moles of water will be produced when 7.0 mol of KMnO4<br />
are used up?<br />
e) What is the maximum mass of Cl2 that can be produced by reacting<br />
35.0 g of KMnO4 with 45.0 g of HCl?
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