Stoichiometric Gram to Gram Calculations Worksheet
 1. The combustion of a sample of butane, C4H10 (lighter fluid), produced 2.46 grams of water. 2 C4H10 + 13 O2 -------> 8 CO2 + 10 H2O (a) How many moles of water formed? (b) How many moles of butane burned? (c) How many grams of butane burned? (d) How much oxygen was used up in moles? In grams? 2. Terephthalic acid, an important raw material for making Dacron, a synthetic fibre,  is made from para-xylene by the following reaction. C8H10 + 3 O2 ------------------------> C8H6O4 + 2 H2O                     para-                special conditions          terephthalic                    xylene                                                          acid How much terephthalic acid could be made from 154 grams of para-xylene in moles? In grams? 3. Adipic acid, a raw material for nylon, is made industrially by the oxidation of cyclohexane. 5 O2 + 2 C6H12         ----------------------> 2 C6H10O4 + 2 H2O                             cyclohexane      special conditions          adipic acid (a)   How many moles of oxygen would be needed to make 40.0 moles of adipic acid by this reaction? (b)   If 164 grams of cyclohexane is used, what is the theoretical yield of adipic acid in moles? In grams? 4. Aluminum oxide, Al2O3, a buffing powder, is to be made by combining 5.00 grams of aluminum with oxygen, O2. How much oxygen is needed in moles? In grams? 5. Calculate how many grams of iron can be made from 16.5 grams of Fe2O3 by the following equation. Fe2O3 + 3 H2 -------------> 2 Fe + 3 H2O 6. Iodine chloride, ICl, can be made by the following reaction between iodine, I2, potassium iodate, KIO3, and hydrochloric acid. 2 I2   +   KIO3  +  6 HCl  --------->   5 ICl  +  KCl  +  3 H2O Calculate how many grams of iodine are needed to prepare 28.6 grams of ICl by this reaction. 7. The nitrite ion (NO2-) in potassium nitrite is changed to the nitrate ion by the action of potassium permanganate (KMnO4) in sulphuric acid solution. 5 KNO2 + 2 KMnO4 + 3 H2SO4 ------>   5 KNO3 + 2 MnSO4 + K2SO4 + 3 H2O How many moles and how many grams of KMnO4 are needed to carry out this reaction on 11.4 grams of KNO2? 8. The chief component of glass is silica for which the formula SiO2 can be used.  Silica is dissolved by hydrofluoric acid, HF, according to the following reaction that produces silicon tetrafluoride, SiF4, a gas at room temperature. SiO2 + 4 HF ------------> SiF4 + 2 H2O How many grams and how many moles of SiF4 can be produced from 63.4 grams of HF? 9. Copper(I) iodide, CuI, is not stable enough to last long in storage, so it is generally made just prior to use. In can be prepared from copper sulphate and hydriodic acid by the following reaction. 2 CuSO4 + 4 HI -------------> 2 CuI + 2 H2SO4 + I2 If 10.4 grams of CuSO4 is used, calculate the number of grams of HI needed and the number of grams of each of the products that are produced. Show that the mass data are in accordance with the law of conservation of mass in chemical reactions. 10. If 2.56 grams of chlorine, Cl2, are to be used to prepare dichlorine heptoxide, Cl2O7, how many moles and how many grams of oxygen are needed? 11. Under the right conditions, ammonia can be converted to nitric oxide, NO by the following reaction. 4 NH3 + 5 O2 -----------> 4 NO + 6 H2O How many moles and how many grams of oxygen are needed to react with 56.8 grams of ammonia by this reaction? 12. One way to prepare iodine is to mix sodium iodate, NaIO3, 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 that can be made this way from 16.4 grams of NaIO3. 13. Nickel metal reacts with silver nitrate solution according to the following balanced equation. Ni + 2 AgNO3 ----------->  2 Ag + Ni(NO3)2 If 15.32 grams of nickel reacts with an excess of silver nitrate solution, calculate the mass of silver produced. 14. How many grams of CO2 are produced when 23 grams of C2H5OH are burned? 15. Given: 3 Fe2O3 + CO -------------> 2 Fe3O4 + CO2 How many grams of Fe2O3 can be converted to Fe3O4 by 14.0 grams of CO?