<p> Stoichiometry Problems: Mixed Bag!!!</p><p>Name ______Date ______Period ______</p><p>Directions: Show all your work as you answer your problems. Remember to include a unit and a substance with your solved for value.</p><p>1) 4 FeCr2O7 + 8 K2CO3 + 1 O2  2 Fe2O3 + 8 K2CrO4 + 8 CO2</p><p>(a) How many moles of FeCr2O7 are required to produce 44 moles of CO2?</p><p>(b) How many moles of O2 are required to produce 107.9 moles of Fe2O3?</p><p>2) Given the reaction S + O2  SO2</p><p>(a) What type of equation is it?</p><p>(b) How many moles of sulfur must be burned to give 0.567 moles of SO2?</p><p>(c) How many moles of SO2 can be produced from 67.1 moles of O2?</p><p>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?</p><p>4) For the reaction 2HNO3 + Mg(OH)2 → Mg(NO3)2 + 2H2O, (a) what type of reaction is it?</p><p>(b) how many grams of magnesium nitrate [Mg(NO3)2] are produced from 8.00 moles of water?</p><p>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)</p><p>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.</p><p>FeCl3(aq) + 3 NaOH(aq)  Fe(OH)3(s) + 3 NaCl(aq)</p><p>7) Calculate the mass of hydrogen gas that will be released when 3.0 g of sodium reacts with water.</p><p>2 Na(s) + 2 H2O(l)  2 NaOH(aq) + H2(g)</p>