Exam Review: Calculations
Date: Friday, June 24 Room: 212 Time: 8:30-10:30 am Marks: 120 (75 multiple choice) % of grade: 30%
You will be given a periodic table (as used for tests), a list of polyatomic ions, the activity series, solubility rules,
EN values, and a list of constants: 6.02x1023, 22.4 L, 24.8 L, 273 K, 101.3 kPa, 8.31 (kPa·L)/(mol·K), 4.18 J/(g·ºC).
Basically, any information that you did not have to memorize for a test, you do not have to memorize for the exam.
This sheet is not a complete review of SCH 3U1 chemistry. You will still need to review all of your notes (especially
focus on unit review sheets). This review is meant to help you sort through the different types of calculations that we
have done. Try to solve these questions first without your notes (after all, you won’t have your notes during the exam).
1. How many electrons, protons, and neutrons are in 19F? Ar-40?
2. What chemical formula results when the following elements are combined: a) Al + S, b) Mg + O?
3. Calculate ΔEN for: NaF, H2O, O2. What kinds of intermolecular forces will result in each case?
4. Calculate the percentage composition (by mass) of H3PO4.
5. 4.89 ÷ 6.77 + 1.2782 x 2.78 = __ (give your answer with the correct number of significant digits).
6. Boron has two isotopes: 10B (19.9%) and 11B (80.1%). Calculate Boron’s average atomic mass.
7. How many atoms are in 7.3 moles of C2H4?
8. How much does 3.8 mol CuSO4 weigh in grams?
9. A compound contains C (63.2% by mass), H (8.8%), and O (28.0%). Calculate its simplest formula.
10. A compound has the simplest formula CH2O and a molar mass of 180 g/mol. Give its molecular formula.
11. Write nuclear equations showing the a) alpha decay of 210Bi, b) beta decay of 75Se.
12. Butane burns according to the equation: 2C4H10 + 13O2 → 8CO2 + 10H2O. If a 10 mL test tube is filled
1/10 with butane and 9/10 with O2, how much O2 will remain at the end of the reaction?
13. 2KNO3 → 2KNO2 + O2. What mass of O2 can be produced from 592