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Final Exam with Answers Key - General Chemistry I | C 150, Exams of Chemistry

South Carolina State University (SCSU)Chemistry

Material Type: Exam; Class: General Chemistry I; Subject: Chemistry; University: South Carolina State University; Term: Unknown 1989;

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South Carolina State University Chapter 3
Department of Biological and Physical Sciences
General Chemistry I, C 150 -07 Hamidi
Multiple Choice: Identify the letter of the choice that best completes the statement or answers the question.
____ 1. What scientific (natural) law serves as the basis for balancing chemical equations by requiring that there be no
observable change in the quantity of matter during a chemical reaction?
a. Law of Conservation of Energy
b. Law of Multiple Proportions
c. Law of Conservation of Matter
d. Law of Definite Proportions
e. Law of Constant Composition
____ 2. Balance the following equation with the smallest whole number coefficients. What is the coefficient for O2
in the balanced equation?
C4H10 + O2 โ†’ CO2 + H2O
a. 9
b. 5
c. 15
d. 6
e. 13
____ 3. What is the coefficient for HBr when the following equation is balanced with the smallest whole number
coefficients?
Br2 + H2O โ†’ HBr + HBrO3
a. 5
b. 7
c. 8
d. 3
e. 6
____ 4. Balance the following equation with the smallest whole number coefficients. What is the coefficient for NH3
in the balanced equation?
Fe(NO3)3 + NH3 + H2O โ†’ Fe(OH)3 + NH4NO3
a. 1
b. 3
c. 2
d. 6
e. 4
____ 5. Elemental phosphorus is produced from calcium phosphate in the following reaction. What is the coefficient
for C when this equation is balanced with the smallest whole number coefficients?
Ca3(PO4)2 + SiO2 + C โ†’ P4 + CO + CaSiO3
a. 10
b. 3
c. 1
d. 6
e. 4
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pf5
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Download Final Exam with Answers Key - General Chemistry I | C 150 and more Exams Chemistry in PDF only on Docsity!

South Carolina State University Chapter 3

Department of Biological and Physical Sciences

General Chemistry I, C 150 -07 Hamidi

Multiple Choice: Identify the letter of the choice that best completes the statement or answers the question.

____ 1. What scientific (natural) law serves as the basis for balancing chemical equations by requiring that there be no observable change in the quantity of matter during a chemical reaction? a. Law of Conservation of Energy b. Law of Multiple Proportions c. Law of Conservation of Matter d. Law of Definite Proportions e. Law of Constant Composition

____ 2. Balance the following equation with the smallest whole number coefficients. What is the coefficient for O 2 in the balanced equation? C 4 H 10 + O 2 โ†’ CO 2 + H 2 O

a. 9 b. 5 c. 15 d. 6 e. 13

____ 3. What is the coefficient for HBr when the following equation is balanced with the smallest whole number coefficients? Br 2 + H 2 O โ†’ HBr + HBrO 3

a. 5 b. 7 c. 8 d. 3 e. 6

____ 4. Balance the following equation with the smallest whole number coefficients. What is the coefficient for NH 3 in the balanced equation? Fe(NO 3 ) 3 + NH 3 + H 2 O โ†’ Fe(OH) 3 + NH 4 NO 3 a. 1 b. 3 c. 2 d. 6 e. 4

____ 5. Elemental phosphorus is produced from calcium phosphate in the following reaction. What is the coefficient for C when this equation is balanced with the smallest whole number coefficients? Ca 3 (PO 4 ) 2 + SiO 2 + C โ†’ P 4 + CO + CaSiO 3

a. 10 b. 3 c. 1 d. 6 e. 4

____ 6. Ultra-pure Si is required to produce semi-conductors. The first step in this process is combining silicon dioxide with carbon and chlorine. Choose the answer that represents the sum of all the coefficients when this equation is balanced the smallest whole number coefficients.

SiO 2 + C + Cl 2 โ†’ CO + SiCl 4

a. 5 b. 6 c. 16 d. 7 e. 8

____ 7. Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one".

PBr 3 + H 2 O โ†’ H 3 PO 3 + HBr

a. 7 b. 8 c. 9 d. 10 e. 11

____ 8. Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one".

CuSO 4 + NH 3 + H 2 O โ†’ (NH 4 ) 2 SO 4 + Cu(NH 3 ) 4 (OH) 2

a. 8 b. 9 c. 11 d. 12 e. 14

____ 9. Consider the following balanced equation.

2H 2 + O 2 โ†’ 2H 2 O

Which one of the following statements is false? a. One molecule of O 2 will react with 2 molecules of H 2. b. One mole of O 2 will react with 2 moles of H 2. c. The complete reaction of 32.0 g of O 2 will produce 2 moles of H 2 O. d. The complete reaction of 2.0 g of H 2 will produce 36.0 g of H 2 O. e. The amount of reaction that consumes 32.0 g of O 2 produces 36.0 g of H 2 O.

____ 10. How many moles of O 2 are required to react with 23.5 moles of methanol?

2CH 3 OH + 3O 2 โ†’ 2CO 2 + 4H 2 O

a. 47. b. 35. c. 11. d. 40 e. 23.

____ 16. If 25.0 g of each reactant were used in performing the following reaction, which would be the limiting reactant?

3PbO 2 + Cr 2 (SO 4 ) 3 + K 2 SO 4 + H 2 O โ†’ 3PbSO 4 + K 2 Cr 2 O 7 + H 2 SO 4

a. PbO 2 b. H 2 O c. K 2 SO 4 d. PbSO 4 e. Cr 2 (SO 4 ) 3

____ 17. How many moles of carbon dioxide could be produced if 10 moles of octane, C 8 H 18 , are combined with 20 moles of oxygen?

C 8 H 18 + 25O 2 โ†’ 16CO 2 + 18H 2 O

a. 40 mol b. 8.0 mol c. 12.8 mol d. 62.5 mol e. 20 mol

____ 18. What mass of ZnCl 2 can be prepared from the reaction of 1.69 grams of zinc with 1.10 grams of HCl?

Zn + 2HCl โ†’ ZnCl 2 + H 2

a. 2.30 g b. 2.27 g c. 2.45 g d. 2.06 g e. 4.11 g ____ 19. What is the percent yield of CO 2 if the reaction of 10.0 grams of CO with excess O 2 produces 12.8 grams of CO 2?

2CO(g) + O 2 (g) โ†’ 2CO 2 (g)

a. 76.4% b. 78.1% c. 81.5% d. 84.4% e. 88.9%

____ 20. Salicylic acid reacts with acetic anhydride to form aspirin, acetylsalicylic acid. If the percent yield in this reaction is 78.5%, what mass of salicylic acid is required to produce 150. g aspirin?

2 C 7 H 6 O 3 + C 4 H 6 O 3 โ†’ 2 C 9 H 8 O 4 + H 2 O salicylic acid acetic anhydride aspirin

a. 292 g b. 146 g c. 90.0 g d. 73.0 g e. 191 g

____ 21. What is the percent yield if 28.50 of FeO reacts with excess CO and produces 17.841 g Fe?

FeO + CO โ†’ Fe + CO 2

a. 62.62% b. 81% c. 80.55% d. 124% e. 77.72%

____ 22. What mass of water is contained in 160. grams of 22.0% KCl solution? a. 125 g b. 86.8 g c. 35.2 g d. 130 g e. 112 g

____ 23. What mass of NaF and water are required to produce 680. g of 15.0 wt % NaF solution? a. 170 g NaF, 510 g H 2 O b. 11 g NaF, 669 g H 2 O c. 578 g NaF, 102 g H 2 O d. 15 g NaF, 665 g H 2 O e. 102 g NaF, 578 g H 2 O

____ 24. What mass of Na 2 SO 4 is required to prepare 400. mL of 1.50 M Na 2 SO 4 solution? a. 213 g b. 56.8 g c. 71.4 g d. 85.2 g e. (^) 8.52 ร— 104 g

____ 25. What volume of 0.250 M KOH solution contains 6.31 grams of KOH? a. 631 mL b. 28.1 mL c. 450 mL d. 2.22 mL e. 0.44 mL

____ 26. The specific gravity of commercial nitric acid solution is 1.42 and it is 70.0% HNO 3 by mass. Calculate its molarity. a. 18.0 M b. 15.8 M c. 12.8 M d. 99.4 M e. 26.2 M

____ 27. A laboratory stock solution is 1.50 M NaOH. Calculate the volume of this stock solution that would be needed to prepare 300. mL of 0.200 M NaOH. a. 2.25 mL b. 10.0 mL c. 40.0 mL d. 1.00 mL e. 0.100 mL

____ 28. When a solution is diluted, what is the relationship of the number of moles of solute in the more concentrated initial volume of solution to the number of moles of solute in the less concentrated final volume of solution?

chapter

Answer Section

MULTIPLE CHOICE

  1. ANS: D TOP: Chemical Equations
  2. ANS: E TOP: Chemical Equations
  3. ANS: A TOP: Chemical Equations
  4. ANS: B TOP: Chemical Equations
  5. ANS: A TOP: Chemical Equations
  6. ANS: E TOP: Chemical Equations
  7. ANS: B TOP: Chemical Equations
  8. ANS: C TOP: Chemical Equations
  9. ANS: D TOP: Calculations Based on Chemical Equations
  10. ANS: B TOP: Calculations Based on Chemical Equations
  11. ANS: C TOP: Calculations Based on Chemical Equations
  12. ANS: E TOP: Calculations Based on Chemical Equations
  13. ANS: D TOP: Calculations Based on Chemical Equations
  14. ANS: C TOP: Calculations Based on Chemical Equations
  15. ANS: C TOP: Calculations Based on Chemical Equations
  16. ANS: A TOP: The Limiting Reactant Concept
  17. ANS: C TOP: The Limiting Reactant Concept
  18. ANS: D TOP: The Limiting Reactant Concept
  19. ANS: C TOP: Percent Yields from Chemical Reactions
  20. ANS: B TOP: Percent Yields from Chemical Reactions
  21. ANS: C TOP: Percent Yields from Chemical Reactions
  22. ANS: A TOP: Concentrations of Solutions
  23. ANS: E TOP: Concentrations of Solutions
  24. ANS: D TOP: Concentrations of Solutions
  25. ANS: C TOP: Concentrations of Solutions
  26. ANS: B TOP: Concentrations of Solutions
  27. ANS: C TOP: Dilution of Solutions
  28. ANS: E TOP: Dilution of Solutions
  29. ANS: B TOP: Using Solutions in Chemical Reactions
  30. ANS: B TOP: Using Solutions in Chemical Reactions
  31. ANS: A TOP: Using Solutions in Chemical Reactions
  32. ANS: B TOP: Using Solutions in Chemical Reactions