Station 1: Significant Figures, Empirical Formulas & Formula Mass

  1. How many sig figs are in:

0.0045 2100.04378030.0402180. 3

  1. Solve and round your answer to the appropriate number of sig figs:

870 + 33.5 – 250.01 + 0.0087 = 650

  1. Solve and round your answer to the appropriate number of sig figs:

0.0980 x 8710 ÷ 74 x 0.05 =0.6

  1. What is the formula mass of magnesium hydroxide?Mg(OH)258.321 g/mol
  1. What is the formula mass of calcium phosphate? Ca3(PO4)2310.188 g/mol

Station 2: Writing Chemical Formulas & Names

  1. Calcium PhosphateCa3(PO4)27. Barium bromide BaBr2
  2. Tricarbonheptahydride C3H78. Zinc phosphide Zn3P2
  3. NiONickel (II) Oxide9. Silver carbonate Ag2CO3
  4. Pb(OH)4Lead (IV) Hydroxide10. Li3N Lithium nitride
  5. Iron (III) chlorideFeCl311. P3F5 Triphosphorous Pentafluoride
  6. Dinitrogen trioxideN2O312. RbI Rubidium Iodide

Station 3: Classifying and Balancing Reactions

Classify each reaction and balance.

  1. Single Displacement Zn + H2SO4 -----> ZnSO4 + H2
  2. Decomposition H2CO3 -----> CO2 + H2O
  3. Double Displacement CaCO3 + 2HCl ------> CaCl2 + H2CO3
  4. Combustion C3H8 + 5O2 -----> 3CO2 + 4H2O
  5. Decomposition H2SO4 -----> H2O + SO3

Write a balanced equation for the following reactions

  1. Magnesium chloride is the product of a reaction between magnesium and chlorine.

Mg + Cl2 MgCl2

  1. A double displacement reaction between potassium hydroxide and copper (II) sulfate.

2KOH + CuSO4 K2SO4 + Cu(OH)2

Station 4: The Mole & Stoichiometry

  1. How many moles are in 8.56 x 1025 atoms of potassium.142 moles
  2. How many moles are 750grams ofhydrogen sulfide. 22 moles
  3. How many grams are in 8.5 moles of carbonic acid. 530 g

Use the following balanced equation to answer questions 4-6

2 SO2(g) + 2 CaCO3(s) + O2(g)  2 CaSO4(s) + 2 CO2(g)

  1. How many moles of carbon dioxide are produced from 25 grams of SO2? 0.39 moles CO2
  2. How many grams of calcium carbonate are used when 156 grams of oxygen gas react? 976g CaCO3
  3. How many moles of calcium sulfate are produced from 17.25 grams of sulfur dioxide?0.2693 mol CaSO4

Station 5: Predicting Products of Reactions

Predict the products of these single displacement reactions and write the balanced equation.

  1. lead + zinc acetate Pb + Zn(C2H3O)  NR
  2. sodium iodide + bromine 2NaI + Br2 2NaBr + I2
  3. iron + aluminum oxide Fe + Al2O3 NR

Predict the products of these double displacement reactions and write the net ionic equations.

  1. 2 AgNO3(aq) + _____ K2CO3(aq) Ag2CO3(s) + 2KNO3(aq)
  1. _____ MgBr2(aq) + 2 KOH (aq) 2KBr(aq) + Mg(OH)2(s)

Station 5: Gas Laws & Solutions

  1. A sample of carbon dioxide occupies a volume of 3.50 Liters at 125 kPa pressure. What pressure would the gas exert if the volume was decreased to 2.00 liters? 219 kPa
  2. How many moles of nitrogen gas will occupy a volume of 347 mL at 6680 mmHg and 27 C?

PV = nRTn = RT/PV0.0821 Latm/molK (27+273) / (6680/760)(.347L)

24.63/3.049947 = 8.1 moles N2

  1. A sample of gas occupies a volume of 450.0 mL at 740 mm Hg and 16°C. Determine the volume of this sample at 760 mm Hg and 37°C.

740 (450) = V (760)V = 470 mL

(16+273) (37+273)

  1. Calculate the molarity of a solution that contains 0.25 moles of HCl in 1.5 L of solution. 0.17 M
  2. How many liters of solution are needed to prepare a 0.1 M solution from 56.0 g sodium carbonate?

5 liters

  1. 20.0 mL of a stock solution of ammonium nitrate is diluted to a final volume of 250.0 mL and a final concentration of 0.150 M. What is the initial concentration (Molarity) of the stock solution?

M1V1 = M2V2 M1(20.0mL) = 0.150M(250.0mL)M1 = 1.88 M

  1. Write the balanced chemical equation for the neutralization reaction between hydrogen bromide and barium hydroxide. 2HBr + Ba(OH)2 BaBr2 + 2H2O

Station 7: Carbon Cycle, Climate Change, Ocean Acidification Diagrams

CO2(g) + H2O(l) + heat  2H+(aq) + CO3-2(aq)
Stress / Shift / [CO2] / [H2O] / [H+] / [CO3-2]
Add CO2(g) / Right / Decrease / Decrease / Increase / Increase
Remove CO3-2(aq) / Right / Decrease / Decrease / Increase / --
Decrease Temperature / Left / Increase / Increase / Decrease / Decrease
Increase Volume / Left / Increase / Increase / Decrease / Decrease
Decrease Pressure / Left / Increase / Increase / Decrease / Decrease