Stoichiometry Problems: Mixed Bag

Stoichiometry Problems: Mixed Bag!!!

Name ______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 FeCr2O7 + 8 K2CO3 + 1 O2  2 Fe2O3 + 8 K2CrO4 + 8 CO2

(a) How many moles of FeCr2O7 are required to produce 44 moles of CO2?

(b) How many moles of O2 are required to produce 107.9 moles of Fe2O3?

2) Given the reaction S + O2  SO2

(a) What type of equation is it?

(b) How many moles of sulfur must be burned to give 0.567 moles of SO2?

(c) How many moles of SO2 can be produced from 67.1 moles of O2?

3) For the reaction C + 2H2 → CH4, (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 2HNO3 + Mg(OH)2 → Mg(NO3)2 + 2H2O, (a) what type of reaction is it?

(b) how many grams of magnesium nitrate [Mg(NO3)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) + O2(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 [FeCl3] reacts with an excess of sodium hydroxide.

FeCl3(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 H2O(l)  2 NaOH(aq) + H2(g)