Name: ________________________ Date: ____________ Period: _______Chemistry Student Learning Objective Review Part 3

Unit 7: Chemical Reactions Chapter 111. Define/describe the following types of reactions

a. Synthesis

b. Decomposition

c. Single Replacement

d. Double Replacement

e. Neutralization

f. Combustion

2. Identifying types of reactions shown below (DO NOT BALANCE REACTOINS) Equation

1. N2 + H2 → NH3

2. KClO3 → KCl + O2

3. C8H18 + O2 → CO2 + H2O

4. NaCl + F2 → NaF + Cl2

5. AgNO3 + MgCl2 → AgCl + Mg(NO3)2

6. CH4 + O2 → CO2 + H2O

7. Sr(OH)2 + HI → SrI2 + H2O

8. C3H6 + O2 → CO2 + H2O

9. FeCl3 + NaOH → Fe(OH)3 + NaCl

10. Na + H2O → NaOH +H2

11. NaOH +HCl → NaCl + H2O

12. Ag2O → Ag + O2

13. S8 + O2 → SO3

14. K + MgBr2 → KBr + Mg

Type of Reaction

1. __________________________

2. __________________________

3. __________________________

4. __________________________

5. __________________________

6. __________________________

7. __________________________

8. __________________________

9. __________________________

10. __________________________

11. __________________________

12. __________________________

13. __________________________

14. __________________________

3. Balance the following reactions and identify the type of reaction (show balancing work)a) ___ Na + NaNO3 Na2O + N2 Type: __________________________

b) ___ N2 + O2 ___ N2O5 Type: __________________________

c) _____H3PO4 + ____Ca(OH)2_____Ca3(PO4)2 + _____H2OType: __________________________

d) ____AlCl3 + ____Na2CO3____Al2(CO3)3 + _____NaCl Type: __________________________

e) _____AlCl3 _____Al + _____Cl2 Type: __________________________

f) _____ C2H6 + _____ O2 → _____ CO2 + _____ H2O Type: __________________________

4. What are the 7 diatomic elements?

5. Turn the following word equations into skeleton equations (don’t balance # of atoms)a) When solid potassium nitrate is heated, it forms solid potassium nitrite and oxygengas.

b) When dissolved sodium hydroxide reacts with sulfuric acid aqueous sodium sulfate and water are formed.

c) zinc metal and oxygen gas react to produce zinc oxide

d) Sodium phosphate and calcium chloride react to form calcium phosphate and sodium chloride.

e) sodium chloride and lead (II) nitrate produce lead (II) chloride and sodium nitrate

f) In a blast furnace, iron (III) oxide and carbon monoxide gas produce carbondioxide gas and iron.

Unit 8& 9:  Chemical Quantities Chapter 10& 126. Find the percent composition for the following problems, show ALL calculations.

a. Percent composition of Chromium in Sn(Cr2O7)2

b. Percent composition of oxygen in calcium acetate

c. Percent composition of Strontium in Sr3N2

7. Define and give example of:a. Empirical formula

b. Molecular formula

8. Empirical/Molecular formula practicea. What is empirical formula for C4H10?

b. What is empirical formula for C12H22O2?

c. A compound with an empirical formula of C4H4O and a molar mass of 136 grams per mole. What is the molecular formula of this compound?

d. Empiricalformula is C2H4NO. If its molar mass is 116.1 g/mol, what is the molecular formula?

9. Complete the following stoichiometric equalities

a. _________ mole = ___________ liters c. _________ mole = _________ grams

b. _________ mole = ____________ particles d. _________ mole = ________ molecules

10. Complete the following conversions showing ALL work with units (including molar mass calculations).

4P(s) + 5O2(g) →2P2O5(s)a. If you have 56.7 g of oxygen how many liter of oxygen do you have?

b. When 276.6 g of phosphorous is reacted with excess oxygen how many grams of P2O5 did you produce?

C2H4+ 3O2→ 2CO2 + 2H2Oc. If you produced 46.56 grams of water how many grams of oxygen did your react?

d. If 12.5 g of C2H4 is reacted with 12.5 g O2 how many grams of CO2 did you produce?

e. 5.75 grams of Iron react with 6.05 grams of Chlorine producing 14.50 grams Iron (III) Chloride.

i. Write a balanced chemical equation for the reaction above

ii. Determine the limiting reactant.

iii. Calculate the theoretical yield of Iron (III) Chloride

iv. Determine the percent yield of Iron (III) Chloride.

f. 12.5 grams of Iodine react with 11.9 grams of Chlorine producing 19.5 grams Iodine Trichloride.i. Write a balanced chemical equation for the reaction above

ii. Determine the limiting reactant.

iii. Calculate the theoretical yield of Iodine Trichloride.

iv. Determine the percent yield of Iodine Trichloride.