Supplemental Instruction
Iowa State University / Leader: / Matt HermsenWhite
Course: / Chem 177
Instructor: / Dr Irmi Schewe-Miller
Date: / 1-5-17
1. In the following list, only ______is not an example of a chemical reaction.
a. dissoulution of penny in nitric acid
b. condensation of water vapor
c. burning a candle
d. formation of polyethylene from ethylene
2. Which famous chemist in 1803 wrote the Atomic Theory describing the nature of matter?
a. Rutherford
b. Dalton
c. Avogadro
d. Mendeleev
3. One mole of which contains the most atoms?
a. hydrogen b. calcium c. silver d. one mole of anything contains the same #
4. Which of these is the highest temperature?
a. 94 ° F b. 39 ° C c. 300 K
5. The following measurements of a pencil were taken by 3 students. The pencil is actually 5 cm long. Which set of measurements represents accuracy, which represents precision, and which represents neither.
[ 3.9, 3.8, 4.0 ] [ 4.2, 6.3, 5.5 ] [ 5.1, 4.8, 5.2 ]
6. What is the difference between a heterogeneous and homogenous mixture?
9. Which of the following is a metalloid?
a. Aluminum b. Silicon c. Sulfur d. Selenium
7. What is the charge on the phosphate ion?
a. -1 b. -2 c. -3 d. neutral
8. What is the formula for Chromium (II) Bromide?
a. CrBr b. CrBr2 c. Cr2Br d. Cr2Br2
9. Fill the table
Charge / Mass (amu) / Location in Atom / When happens to atom when you change amountProton
Neutron
Electron
10. Which atom has the largest number of neutrons?
a. Argon – 40
b. Potassium – 39
c. Calcium – 40
d. Chlorine – 35
11. List the seven diatomic molecules
12. Name the following polyatomic ions
CO4 2-
CO3 2-
CO2 2-
CO2 -
13. Write name or chemical formula for the following. Are they ionic or molecular?
a. N2O5
b. Barium Sulfite
c. NBr3
d. Hydroiodic Acid
e. NaClO
f. LiOH
g. MgSO3
h. Fe2(CO3)3
i. HClO4
j. Hypochloric acid
k. P2O5
l. Lithium Fluoride
m. Chromium (III) Acetate
14. What is the percent composition by mass of O in dinitrogen pentoxide?
15. Convert 65 mph to m/s. (1 mi = 5280 ft) (3.3 ft = 1 m)
16. When the following equation is balanced, the coefficients are ______.
a. 2, 3, 4, 4 b. 1, 4, 8, 9 c. 2, 12, 8, 9 d. 2, 25, 16, 18
C8H18 + O2 à CO2 + H2O
17. What type of reaction is the problem above?
18. Chlorine has an average atomic mass of 35.45 amu, which is calculated from the two isotopes of Cl. Isotope A: 34.969 amu Isotope B: 36.966
What are the percent compositions in nature of isotope A and B?
19. Adrenaline is composed of 4 elements. C: 59.0% H: 26.2% O: 26.2% N: 7.7% by mass. Its molar mass is about 180 g/mol.
What are the empirical and molecular formulas for adrenaline?
20. Count the total number of atoms in .111 mol Fe(CO)3(PH3)2
21. How many hydrogen atoms are in 10 g of CH3COOH (acetic acid)?
22. How much does 100 million atoms of copper weigh?
23. A certain factory has a 93.50% success rate in converting Silver Nitrate into pure silver. In one day it creates 630. kg of pure silver. What is the factory’s theoretical yield for one day’s processing of silver?
24. A certain box contains 6.0 kg of water. The box width and height are 18 cm and 15 cm respectively. What is the height of the box?
25. The following is a step in the commercial process of converting ammonia into nitric acid.
4NH3 (g) + 5 O2 (g) à 4NO (g) + 6H2O (g)
In this experiment, 2.00 g of NH3 reacts with 2.50 g of O2.
a. How many grams of NO and H2O are produced?
b. How many grams of excess reactant remain?
26. A solution of ammonia and water contains 2.10 x 1025 water molecules, and 8.10 x 1024 ammonia molecules. How many total hydrogen atoms are in the solution?