Name _____________________
Stoichiometry Problems: Mixed Bag!!!
Date ______ Period _______
Directions: Show all your work as you answer your problems. Remember to include a unit and a substance with your solved for value.
1) 4 FeCr
2
O
7
+ 8 K
2
CO
3
+ 1 O
2
 2 Fe
2
O
3
+ 8 K
2
CrO
4
+ 8 CO
2
(a) How many moles of FeCr
2
O
7
are required to produce 44 moles of CO
2
?
(b) How many moles of O
2
are required to produce 107.9 moles of Fe
2
O
3
?
2) Given the reaction S + O
2
 SO
2
(a) What type of equation is it?
(b) How many moles of sulfur must be burned to give 0.567 moles of SO
2
?
(c) How many moles of SO
2
can be produced from 67.1 moles of O
2
?
3) For the reaction C + 2H
2
→ CH
4
,
(a) what type of reaction is it?
(b) how many grams of hydrogen are required to produce 0.6 moles of methane, CH4?
4) For the reaction 2HNO
3
+ Mg(OH)
2
→ Mg(NO
3
)
2
+ 2H
2
O,
(a) what type of reaction is it?
(b) how many grams of magnesium nitrate [Mg(NO
3
)
2
] are produced from 8.00 moles of water?
5) Calculate the mass of magnesium oxide (MgO) formed when 0.52 g of magnesium is burned according to the following equation: 2 Mg
(s)
+ O
2(g)

2 MgO
(s)
6) Determine the mass of iron(III) hydroxide [Fe(OH)
3
]which should form when a solution containing 3.00 g of iron(III) chloride [FeCl
3
] reacts with an excess of sodium hydroxide.
FeCl
3(aq)
+ 3 NaOH
(aq)

Fe(OH)
3(s)
+ 3 NaCl
(aq)
7) Calculate the mass of hydrogen gas that will be released when 3.0 g of sodium reacts with water.
2 Na
(s)
+ 2 H
2
O
(l)

2 NaOH
(aq)
+ H
2(g)