Name: ______Date: ______Period: ______

Unit 6 Test Study Guide – Mole & Stoichiometry

Balancing Equations: Balance each of the following chemical equations by writing the correct number on the blanks provided.

  1. _____Na +_____O2  _____Na2O4. _____Ti + _____Fe3O4_____Ti2O3 + _____Fe
  1. _____K2S + _____O2 _____K2O + _____SO25. _____C4H10 + _____O2_____CO2 + _____H2O
  1. _____Mg(NO3)2 + _____NaI _____MgI2 + _____NaNO3

Mole Calculations

  1. Calculate the number of molecules present in 35.7 L of carbon dioxide gas at STP.
  1. How many grams are present in a 0.675 mole sample of iron(III) hydroxide?
  1. How many liters of hydrogen gas are equal to 3.01 x 1023 molecules of hydrogen (H2)?

Stoichiometry Calculations & Percent Yield & Limiting Reagent

  1. Burning coal and oil in a power plant produces pollutants such as sulfur dioxide, SO2. The sulfur-containing compound can be removed from other waste gases, however, by the following balanced equation:

2 SO2(g) + 2 CaCO3(s) + O2(g)  2 CaSO4(s) + 2 CO2(g)

  1. How many moles of Sulfur dioxide can be made from 35.2 grams of carbon dioxide?
  1. What mass of CaCO3 is required to remove 250.0 g of SO2?
  1. If 500.0 g of CaCO3 is used, calculate the percent yield if 195 g of carbon dioxide is actually yielded. (hint-first calculate the theoretical yield of carbon dioxide using stoichiometry)
  1. The black oxide of iron, Fe3O4, occurs in nature as the mineral magnetite. This substance can also be made in the laboratory by the reaction between red-hot iron and steam according to the balanced equation:

3Fe(s) + 4H2O(g)  Fe3O4(s) + 4H2(g)

  1. When 36.0 g of H2O is mixed with 67.0 g of Fe, which is the limiting reagent?
  1. What mass, in grams, of black iron oxide (Fe3O4) is produced?
  1. Consider the reaction: I2O5(g) + 5 CO(g)  5 CO2(g) + I2(g)
  1. 80.0 grams of Iodine (V) oxide, I2O5, reacts with 28.0 grams of carbon monoxide, CO. Determine the mass of I2 which could be produced?
  1. If, in the above situation, only 0.160 moles of iodine was produced…
  1. What mass of iodine was produced?
  1. What percentage yield of iodine was produced (use the theoretical from question 13a.
  1. Zinc and sulfur react to form zinc sulfide according to the equation: ____ Zn + _____S  ______
  1. If 25.0 gram of zinc and 30.0g of sulfur are mixed,
  2. Which chemical is the limiting reagent?
  1. How many grams of ZnS will form?