Exam 1 Review
Supplemental Instruction
Iowa State University / Leader: / Grady
Course: / Chem 177
Instructor: / Appy
Date: / 02/07/15

Review:

Mass spectrometer – pg. 52 Figure 2.11

Scientists and their experiments and discoveries

Polyatomic ions

Unit prefixes (i.e. centi)

  1. Which of the following is NOT a chemical reaction?

a)Dissolution of penny in nitric acid

b)Burning of a candle

c)The melting of copper

d)Formation of polyethylene from ethylene

  1. How long is the pencil?
  1. You are running an experiment to determine the amount of carbon in a 10g of a liquid. The accepted value of carbons is 5g. Label each of the following a certain level of accuracy and precision. (good or bad)

-4.0g, 1.9g, 9.9g, 8.3g

-3.3g, 3.2g, 3.0g, 3.2g

-5.1g, 5.0g, 4.9g, 5.2g,

  1. Give an example of a homogenous and heterogeneous mixture? How are they different? Also, would CO2 be a mixture?
  1. Label the metals, nonmetals, and metalloids. Give a few properties of metals and nonmetals.

  1. Give the number of sig figs in the following

254 100070 .00951.00550.002500 1710019100.0

  1. Round the final answers in each of the following to the appropriate sig figs:

84.0 + 37.56 =

78.223 * 32.2 =

23.34(78.4) + 18.99 =

8.`Fill in the following table:

Charge / Approx. mass (amu) / Location in atom / # in neutral carbon atom / If number changes the element becomes a/an…
Proton
Neutron
Electron
  1. Write number of protons, neutrons, atomic mass, and electrons.
  1. Write the name or chemical formula for each compound. Say whether its molecular or ionic.

Butane

Heptane

Calcium Acetate

Ferric iodide

Silver phosphate

Lead (II) Carbonate

Dinitrogen Tetroxide

HF

Nitrous acid

Phosphorous acid

HCl

HClO

Ammonium nitrate

Aluminum chloride

P2O5

Ti(C2H3O2)3

P3I

  1. Name these ions and the acid they would become.

SO52-

SO42-

SO32-

SO22-

  1. Automobile batteries contain sulfuric acid, which is commonly referred to as battery acid. Calculate the number of grams of sulfuric acid in 1.00 gallon of battery acid if the solution has a density of 1.28 g/ml and is 38.1% sulfuric acid by mass. (1 Gallon is 3.78541 L)
  1. A 32.65 g sample of solid is placed in a flask. Toluene, in which the solid is insoluble is added to the flask so that the total volume of the solid and liquid together is 50.00mL. The solid and toluene together weigh 58.58g. The density of the toluene at the temperature of the experiment is .864 g/mL. What is the density (in kg/m3) of the solid?
  1. Rubidium has two naturally occurring isotopes, 85Rb (relative mass 84.9118 amu) and 87Rb (relative mass 86.9092 amu). If rubidium has an average atomic mass of 85.47 amu, what is the abundance of each isotope (in percent)?
  1. What is the percent of carbon by mass in acetic acid?
  1. Epinephrine (adrenaline), a hormone secreted into the bloodstream in times of danger or stress, contains 59.0% C, 7.1% H, 26.2% O, and 7.7% N by mass; its molecular weight is about 180amu. Give its empirical and molecular formulas.
  1. Combustion analysis of toluene, a common organic solvent, gives 5.86 g of CO2, and 1.37g of H2O. If the compound contains only carbon and hydrogen; its molecular weight is 184 amu.Give its empirical and molecular formulas?
  1. Complete and balance the following reactions: What two reaction types are not included?
  2. Combination

___N2 + ___K 

  1. Decomposition

___Al2O3 

  1. Combustion

___C3H8 + ___O2

  1. 78.34g of carbon is equivalent to how many molecules of carbon?
  1. Hydrogen Sulfide is an impurity in natural gas that must be removed. One common removal method is called the Claus process, which relies on reacting hydrogen sulfide with oxygen both as gases. This produces (l) and water. Under optimal conditions the Claus process gives 98% yield of from Hydrogen Sulfide. If you started with 30.0g of hydrogen sulfide and 50.0g of oxygen, how many grams of would be produced, assuming 98% yield.
  1. The length and width of a box, respectively, 18 cm and 15 cm. If the box holds 6.0 kg of water, what is the height of the box? (water density = 1.0 g/ml)
  1. If 15 grams of copper (II) chloride react with 25. grams of sodium nitrate to produce sodium chloride and copper (II) nitrate, how much sodium chloride can be formed? What is the limiting reactant? If 11.3 grams of sodium chloride are formed in the reaction, what is the percent yield? How much excess reactant remains?Write the balanced chemical reaction