Name _________________________________ Date _________________ Per. ________
HW#36 Stoichiometric calculations in-class worksheet B (Use a calculator)
1. The octane present in gasoline burns according to the following equation:
2 C8H18 + 25 O2 ---------> 16 CO2 + 18 H2O
(octane)
(a) How many moles of O2 are needed to react fully with 4 moles of octane?
(b) How many moles of CO2 can form from 0.5 mole of octane?
(c) How many moles of water are produced by the combustion of 6 moles of octane?
(d) If this reaction is to be used to synthesize 8 moles of CO2, how many moles of oxygen are
needed? How many moles of octane?
2. One way to change iron ore, Fe2O3, into metallic iron is to heat it together with hydrogen.
Fe2O3 + 3 H2 -----------> 2 Fe + 3 H2O
(a) How many moles of iron, Fe, are made from 25 moles of Fe2O3?
(b) How many moles of hydrogen, H2, are needed to make 30 moles of Fe?
(c) How many moles of hydrogen, H2, are needed to make 250 grams of Fe?
3. One way to prepare iodine is to mix sodium iodate, NaIO 3, with hydriodic acid, HI. The
following reaction occurs.
NaIO3 + 6 HI ------------> 3 I2 + NaI + 3 H2O
Calculate the number of moles and the number of grams of iodine, I2, that can be made this
way from 16.4 grams of NaIO3.
4. Nickel metal reacts with silver nitrate, AgNO3, solution according to the following balanced
equation.
Ni + 2 AgNO3 -----------> 2 Ag + Ni(NO3)2
If 15.32 grams of nickel, Ni, reacts with an excess of silver nitrate, AgNO3, solution,
calculate the mass of silver, Ag, produced.
5. Iodine chloride, ICl, can be made by the following reaction between iodine, I2, potassium
iodate, KIO3, and hydrochloric acid, HCl.
2 I2 + KIO3 + 6 HCl ---------> 5 ICl + KCl + 3 H2O
Calculate how many grams of iodine, I2, are needed to prepare 28.6 grams of ICl by this
reaction.
1a) 50 mol O2 b) 4 mol CO2 c) 54 mol H2O d) 12.5 mol O2 and 1 mol C8H18 2a) 50 mol Fe b) 45 mol H2 c) 6.71 mol H2 3) 0.249 mol I2 and 63.1 g of I2 4) 56.32 g Ag 5) 17.88 g I2