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Final Exam ReviewUnits 5-8
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Warm Up
• Go to the blog• Click on the Day 2 WARM UP Questions• While you are waiting to begin, review your
stations from yesterday.
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Station 1 (Moles Unit 5)
• Complete the below Mole Map:
Mole
Volume
MassParticles
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Station 1 (Moles Unit 5)
• Complete the below Mole Map:
Mole
Volume
MassParticles
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Station 1 (Moles Unit 5)
Convert 4.5 g CO2 to molecules.
a) 6.2x1020 moleculesb) 6.2x1022 moleculesc) 1.2x10-25 moleculesd) 1.2x1025 molecules
Calculate the mass of 4.3L of oxygen gas.
a) 3.1 gramsb) 6.1 gramsc) 31 g ramsd) 61 gramse) 138 grams
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Station 1 (Moles Unit 5)
Convert 4.5 g CO2 to molecules.
a) 6.2x1020 moleculesb) 6.2x1022 moleculesc) 1.2x10-25 moleculesd) 1.2x1025 molecules
Calculate the mass of 4.3L of oxygen gas.
a) 3.1 gramsb) 6.1 gramsc) 31 g ramsd) 61 gramse) 138 grams
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Station 2 (Moles Unit 5)
1. Define molecular formula.2. Define empirical formula.3. How do you find empirical formula given the
percent composition? (remember the rhyme)4. Once you have empirical formula how do you
find molecular formula? What other information do you need?
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Station 2 (Moles Unit 5)
1. The actual formula of the compound2. The formula of the compound with reduced
subscripts. Its based on the percent composition.3. % to grams; gram to mole; divide by smallest;
multiply till whole4. Find the molar mass of the empirical formula and
compare it to the given molar mass of the compound (this is the additional information you need). If different, multiply subscripts by their quotient.
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Station 2 (Moles Unit 5)
A compound consisting of C, H, and O is found to contain 40.00% C and 6.71% H. Determine the empirical formula of the compound.
a) CH2O
b) CHOc) C2H4O2
d) C6H12O6
e) CH2
The molecular mass of the compound to the left is calculated to be 180.0 g/mol. Determine the molecular formula of the compound.
a) CH2O
b) C3H6O3
c) C2H4O2
d) C6H12O6
e) C18H36O18
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Station 2 (Moles Unit 5)
A compound consisting of C, H, and O is found to contain 40.00% C and 6.71% H. Determine the empirical formula of the compound.
a) CH2O
b) CHOc) C2H4O2
d) C6H12O6
e) CH2
The molecular mass of the compound to the left is calculated to be 180.0 g/mol. Determine the molecular formula of the compound.
a) CH2O
b) C3H6O3
c) C2H4O2
d) C6H12O6
e) C18H36O18
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Station 3 (Stoichiometry Unit 6)
1. What conversion factor do you use to convert between moles of different elements within a given reaction?
2. What do you need to make sure is done before you use the above factor?
3. How do you determine the limiting reactant?
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Station 3 (Stoichiometry Unit 6)
1. Mole ratio2. Balanced equation3. Solve the stoichiometry problem to find the
mass of the product for each given reactant. The number that gives you the smallest answer is the limiting reactant.
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Station 3 (Stoichiometry Unit 6)P4 + 5O2 P4O10
Determine the mass of tetraphosphorus decoxide formed if 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined.a) 57.3 grams of P4O10
b) 88.7 grams of P4O10
c) 146 grams of P4O10
d) 25.0 grams of P4O10
e) 50.0 grams of P4O10
Which reactant is limiting in the example to the left?
a) 25.0 g of P4
b) 50.0g of O2
c) 57.3 g of P4O10
d) 88.7 grams of P4O10
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Station 3 (Stoichiometry Unit 6)P4 + 5O2 P4O10
Determine the mass of tetraphosphorus decoxide formed if 25.0 g of phosphorus (P4) and 50.0 g of oxygen gas are combined.a) 57.3 grams of P4O10
b) 88.7 grams of P4O10
c) 146 grams of P4O10
d) 25.0 grams of P4O10
e) 50.0 grams of P4O10
Which reactant is limiting in the example to the left?
a) 25.0 g of P4
b) 50.0g of O2
c) 57.3 g of P4O10
d) 88.7 grams of P4O10
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Station 4 (Heat Unit 7)
1. What is the equation that relates heat to change in temperature?
2. Define endothermic3. Define exothermic
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Station 4 (Heat Unit 7)
1. Q=mcΔT2. Endothermic requires heat to be added to
proceed3. Exothermic releases heat
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Station 4 (Heat Unit 7)
• Which of the following is an endothermic phase change?
a) Sublimationb) Freezingc) Condensationd) None of these
• Which of the following is an exothermic phase change?
a) Evaporationb) Meltingc) Depositiond) None of these
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Station 4 (Heat Unit 7)
• Which of the following is an endothermic phase change?
a) Sublimationb) Freezingc) Condensationd) None of these
• Which of the following is an exothermic phase change?
a) Evaporationb) Meltingc) Depositiond) None of these
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Station 4 (Heat Unit 7)
How much heat does a 3.0 grams of water absorb as its temperature increases from 0C to 5.0C?
a) 88.54 Jb) 3.59 Jc) 20.92 Jd) 62.76 J
A 25 g sample of water is absorbs 942 J as it is heated. If the initial temperature of the water was 23.5oC, what is the final temp?a. 9.01 oCb. 32.51 oCc. 157.7 oCd. 134.15 oC
cice=2.1 J/goC, cwater=4.184 J/goC, csteam=1.7 J/goC
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Station 4 (Heat Unit 7)
How much heat does a 3.0 grams of water absorb as its temperature increases from 0C to 5.0C?
a) 88.54 Jb) 3.59 Jc) 20.92 Jd) 62.76 J
A 25 g sample of water is absorbs 942 J as it is heated. If the initial temperature of the ethanol was 23.5oC, what is the final temp?a. 9.01 oCb. 32.51 oCc. 157.7 oCd. 134.15 oC
cice=2.1 J/goC, cwater=4.184 J/goC, csteam=1.7 J/goC
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Station 5 (Solutions Unit 8)
1. What factors affect the rate of solvation (ie. the rate at which a solvent dissolves)?
2. Define molarity. What are its units?3. Define molality. What are its units?
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Station 5 (Solutions Unit 8)
1. Agitation (stirring), increasing temperature (heating), increasing surface area (crushing), all increase the rate of solvation.
2. . It has units of mol/L or M.3. . It has units of mol/kg or m.
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Station 5 (Solutions Unit 8)
What is the volume of solution if the molarity is 0.45M and 0.15 moles of solute are dissolved?
a) 0.33 L of solutionb) 0.33 mL of solutionc) 3.00 L of solutiond) 3.00 mL of solutione) None of these
Calculate the molarity of a solution if 1500 g of H2SO4 is dissolve in 5.0L of water.
a. 300 Mb. 0.3 Mc. 3.06 Md. 0.003 M
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Station 5 (Solutions Unit 8)
What is the volume of solution if the molarity is 0.45M and 0.15 moles of solute are dissolved?
a) 0.33 L of solutionb) 0.33 mL of solutionc) 3.00 L of solutiond) 3.00 mL of solutione) None of these
Calculate the molarity of a solution if 1500 g of H2SO4 is dissolve in 5.0L of water.
a. 300 Mb. 0.3 Mc. 3.06 Md. 0.003 M
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Station 5 (Solutions Unit 8)
What is the mass of NaOH needed to prepare a 3500mL solution of 0.66 M NaOH?
a. 2310 gb. 92.4 gc. 0.0924 gd. 2.31 g
What is the volume of a 0.56M solution containing and 80 grams of NaOH?
a. 3.57 Lb. 35.7mLc. 142.8 Ld. 14.3 L
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Station 5 (Solutions Unit 8)
What is the mass of NaOH needed to prepare a 3500mL solution of 0.66 M NaOH?
a. 2310 gb. 92.4 gc. 0.0924 gd. 2.31 g
What is the volume of a 0.56M solution containing and 80 grams of NaOH?
a. 3.57 Lb. 35.7mLc. 142.8 Ld. 14.3 L
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Station 6 (Acid/Base Unit 8)
1. What is the Arrhenius definition of an acid?2. What is the Arrhenius definition of a base?3. What is the Bronstead-Lowry definition of an
acid?4. What is the Bronstead-Lowry definition of a
base?
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Station 6 (Acid/Base Unit 8)
1. Produces H+ ion2. Produces OH- ion3. H+ ion donor4. H+ ion acceptor
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Station 6 (Acid/Base Unit 8)
According to the Arrhenius theory a substance that releases a hydrogen ion is classified as a(n)
a) Acidb) Basec) Conjugate Acidd) Conjugate Base
Consider the reaction:NH3(aq) + H2O(l) NH4
+(aq) + OH-(aq)
What species is the conjugate acid?
a) NH3
b) H2O
c) NH4+
d) OH-
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Station 6 (Acid/Base Unit 8)
According to the Arrhenius theory a substance that releases a hydrogen ion is classified as a(n)
a) Acidb) Basec) Conjugate Acidd) Conjugate Base
Consider the reaction:NH3(aq) + H2O(l) NH4
+(aq) + OH-(aq)
What species is the conjugate acid?
a) NH3
b) H2O
c) NH4+
d) OH-
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Station 7 (Acid/Base Unit 8)
• What is the pH range for an acid? Base?• Complete the following map:
[H+] pH
[OH-] pOH
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Station 7 (Acid/Base Unit 8)
• What is the pH range for an acid? Base?• Complete the following map:
[H+] pH
[OH-] pOH
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Station 7 (Acid/Base Unit 8)
If the [H+] is equal to 9.2 x 10 -4 M, it’s a(n) _________
a) Acidb) Basec) Neutral solution
Calculate the [OH-] for a solution that has [H+] is equal to 2.0 x 10 -8 M
a. 5.0 x 10-1 Mb. 5.0 x 10-7 Mc. 1.0 x10-7 Md. 2.0 x 10-7 M
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Station 7 (Acid/Base Unit 8)
If the [H+] is equal to 9.2 x 10 -4 M, it’s a(n) _________
a) Acidb) Basec) Neutral solution
Calculate the [OH-] for a solution that has [H+] is equal to 2.0 x 10 -8 M
a. 5.0 x 10-1 Mb. 5.0 x 10-7 Mc. 1.0 x10-7 Md. 2.0 x 10-7 M