Supplemental Instruction
Iowa State University / Leader: / Sara
Course: / Chem 177D
Instructor: / Bonaccorsi
Date: / 9/23/13
1. You weigh a container and its mass is 64.3 grams. It is then filled with water and its new mass is 114.9 grams. What is the volume of the container?
a. 51 mL
b. 50.6 cm3
c. 50.69 cm3
d. 50 mL
2. What is the correct formula for iron (III) Phosphate?
a. Fe2(PO4)3
b. Fe3(PO4)3
c. FePO4
d. Fe3(PO4)2
3. Hydrofluric acid is a clear liquid that had a density of 5.3 g/mL. At room temperature it reacts with silicon dioxide which has a melting point of 1600 degrees Celsius. In the reaction liquid water and silicon tetrafluoride (with a boiling point of -86 degree Celsius) is produced.
a. Write a balanced chemical equation for this reaction and be sure to include states.
4 HF (l) + SiO2 (s) à 2 H2O (l) + SiF4 (g)
b. List 1 chemical, 1 intrinsic and 1 physical property from the above description.
Chemical: HF reacts with SiO2
Physical: melting point and boiling point
Intrinsic: density
4. What is the molar mass of propanol (C3H7OH)?
a. 44 g
b. 46 amu
c. 60 g
d. 46 g
e. 60 amu
5. What is the sum of all the coefficients after the equation is balanced? _2__H3PO4 + _3__Mg(OH)2 à _1__Mg3(PO4)2 + _6__H2O
a. 10
b. 11
c. 12
d. 13
e. 14
6. Which of the following acid’s name and formula is NOT correctly paired?
a. HCl Hydrochloric acid
b. H2SO3 Persulfuric acid
c. H2CO3 Carbonic Acid
d. HNO2 Nitrous Acid
e. H3PO4 Phosphoric acid
7. Solve the equation with the correct amount of significant figures: (10.5734 x 11.527) + 1.3
a. 100
b. 120
c. 123.179
d. 123.18
e. 123.2
8. What is the chemical formula for the ionic compound form from the stable ion of Barium and Arsenic?
a. BaAs3
b. Ba2As3
c. Ba3As2
d. BaAs2
e. BaAs
9. What is the mass of a single molecule of calcium carbonate?
a. 102 Amu
b. 102 g
c. 162 Amu
d. 162 g
10. Wine is a ______
a. Pure substance
b. Homogeneous mixture
c. Heterogeneous mixture
d. Compound
11. Which of the following are chemical properties?
I. flammable
II. reacts with O2
III. melting point at 400 K
a. I only
b. I and II
c. II and III
d. I and III
e. All of them are
12. What is the charge of a proton, neutron and electron respectively?
a. +,-,0
b. -,+,0
c. 0,+,-
d. 0,-,+
e. +,0,-
13. What is NOT a diatomic element?
a. Nitrogen
b. Chlorine
c. Flourine
d. Carbon
e. Hydrogen
Use the periodic Table to answer the next 3 questions:
14. What letter element is a noble gas?
F
15. What letter element is an alkali metal?
A
16. What letter element could have multiple charges
C
17. There are 2 isotopes of Sodium 22Na and 23Na. Their percent abundance is 1.02% and 98.98 % respectively, what is its atomic mass (ignore sig figs)?
(22*1.02/100) + (23*98.98/100)= 22.9898 g/mol
a. If you combine Na with Cl (which also has 2 isotopes 35Cl and 37Cl) how many different combinations of NaCl would show up on a mass spectroscopy chart (show all possibilities)
4
22Na—35Cl
23Na—35Cl
22Na—36Cl
23Na—36Cl
18. You run a 5.0k race in 32 min, what speed were you going in miles/hour (1600 meters in a mile)
5.0 km | 60 min | 1000 m | 1 mile _ = 5.9 miles/hour
32 min | 1 hour | 1 km | 1600 m
19. If you have 24 g of Al2O3, how many atoms of Aluminum do you have?
24 g Al2O3 | 1 mol Al2O3 | 2 mol Al | 6.022 * 1023 molecules = 2.8 * 1023 molecules
| 102 g Al2O3 | 1 mol Al2O3 | mol
20. If 50. g of sulfur dioxide (mm=64.07) reacts with 25 grams of water (mm=18.02) to for sulfurous acid (mm=82.07)
a. What is the chemical equation?
SO2 (s) + H2O (l) à H2SO3 (aq)
b. What is the limiting reagent? SO2
50 g SO2 | 1 mol SO2 | _ = .78 this number is smaller so it is limiting
64.07 g SO2 | 1 mole (molar ratio)
25 g H2O | 1 mol H2O | _ =1.39
18.02 g H2O | 1 mole (molar ratio)
c. How many grams of sulfurous acid is produced?
50 g SO2 | 1 mol SO2 | 1 mol H2SO3 | 82.07 g H2SO3 = 64 g
64.07 g SO2 | 1 mole SO2 | 1 mol H2SO3
d. If the volume of sulfurous acid is 40 cm3 what is the density?
1 g = 1 cm3
D=g/V=64 g / 40 mL = 1.6 g/mL
21. Write the empirical formula for HMn2(NO3)2H3. And calculate the percent composition by mass of each of the elements.
H2MnNO3 119 g/mol
4 Hydrogen 100*(2*1.01)/119 = 1.68 %
2 Manganese 100*(1*55.0)/119 = 46.2%
2 Nitrogen 100*(1*14.0)/119 = 11.6%
6 Oxygen 100*(3*16.0)/119 = 40.3%
22. You combust liquid C2H4 ?
a. What is the chemical equation?
C2H4 (l) + 3O2 (g) à 2CO2 (g) + 2H2O (g)
b. You produce 20.0 grams of carbon dioxide, how much water was produced?
20 g CO2 | 1 mol CO2 | 2 mol H2O | 18 g H2O | = 8.18 g H2O
44 g CO2 | 2 mole CO2 | 1 mol H2O |
c. If you have .50 moles of C2H4 and 1.0 moles of O2 did the reaction go to completion?
.5 mol C2H4 | 2 mole CO2 | 44 g CO2 = 44 g CO2
1 mol C2H4 | 1 mol CO2
1 mol O2 | 2 mole CO2 | 44 g CO2 = 29 g CO2
3 mol O2 | 1 mol CO2
d. In lab you produced .39 moles of carbon dioxide, what was your percent yield?
20 g CO2 | 1 mol CO2 = .455 mol CO2
44 g CO2
.39 mol * 100 = 86 %
.455 mol
23. Fill in the table:
symbol / 19F1- / 32O / 52Cr2+Protons / 9 / 16 / 24
Neutrons / 10 / 16 / 28
Electrons / 11 / 16 / 22
Charge / -1 / 0 / 2+
24. Fill in the blanks in the table:
Compound name / Compound formula / Ionic, covalent or acid?Iron(II) Chloride / FeCl2 / Ionic
Sulfur Tetrabromide / SBr4 / Covalent
Hydroflouric acid / HF / Acid
Sodium Nitrate / NaNO3 / Ionic
Hypoiodous acid / HIO / Acid
Hexanitrogen Monochloride / N6Cl / Covalent