General Chemistry Practice Quiz
General Chemistry Practice Quiz
1. In a dilute solution of sodium chloride in water, the sodium chloride is the
2. A sample of nitrogen at 20° C in a volume of 875 mL has a pressure of 730 mm Hg. What will be its pressure at 20° C if the volume is changed to 955 mL?
a. 750 mm Hg
b. 658 mm Hg
c. 797 mm Hg
d. 669 mm Hg
3. A mixture consisting of 8.0 g of oxygen and 14 g of nitrogen is prepared in a container such that the total pressure is 750 mm Hg. The partial pressure of oxygen in the mixture is
a. 125 mm Hg.
b. 500 mm Hg.
c. 135 mm Hg.
d. 250 mm Hg.
4. To prepare 100 ml of 0.20 M NaCl solution from stock solution of 1.00 M NaCl, you should mix
a. 20 mL of stock solution with 80 mL of water.
b. 40 mL of stock solution with 60 mL of water.
c. 20 mL of stock solution with 100 mL of water.
d. 25 mL of stock solution with 75 mL of water.
5. How many grams of NaOH would be needed to make 250 mL of 0.200 M solution? (molecular weight of NaOH = 40.0)
a. 8.00 g
b. 4.00 g
c. 2.00 g
d. 2.50 g
6. The number of moles of NaCl in 250 mL in a 0.300 M solution of NaCl is
7. A substance has the formula MgSO47H2O. How many grams of water are in 5.00 moles of this substance?
8. How many grams of sugar are needed to make 500 mL of a 5% (weight/volume) solution of sugar?
9. What are the spectator ions in the following equation?
Pb(NO3)2(aq) + 2KCl(aq) → PbCl2(s) + 2KNO3(aq)
a. Pb2+, 2NO3–, 2K+, and 2Cl–
b. Pb2+ and 2NO3–
c. Pb2+, 2K+, and 2Cl–
d. 2NO3– and 2K+
10. What are the products of the following equation?
sodium chloride(aq) + lead(II) nitrate(aq)→
a. sodium nitrate + lead(II) chloride
b. sodium + chloride
c. sodium + chloride + lead(II) + nitrate
d. sodium(II) nitrate + lead chloride
11. Complete the following precipitation reaction:
Hg2(NO3)2(aq) + KI(aq)→
a. Hg2I2(s) + 2K+(aq) + 2NO3–(aq)
b. Hg2I2(s) + 2KNO3(s)
c. Hg22+(aq) + 2NO3–(aq) + 2K+(aq) + 2I–(aq)
d. Hg22+(aq) + 2NO3–(aq) + 2KI(s)
12. Which of the following is NOT true of reversible chemical reactions?
a. A chemical reaction is never complete.
b. The products of the reaction also react to reform the original reactants.
c. When the reaction is finished, both reactants and products are present in equal amounts.
d. The reaction can result in equilibrium.
13. Which is an example of an exothermic change?
14. Which is an example of an endothermic change?
15, The following reaction is exothermic: AgNO3+ NaCl AgCl + NaNO3. How will the equilibrium be changed if the temperature is increased?
a. Equilibrium will shift to the right.
b. Equilibrium will shift to the left.
c. The reaction will not proceed.
d. Equilibrium will not change.
16. The pH of a blood sample is 7.40 at room temperature. The pOH is therefore
c. 6 * 10–6.
d. 4 * 10–7.
17. As the concentration of a hydrogen ion in a solution decreases,
a. the pH numerically decreases.
b. the pH numerically increases.
c. the product of the concentrations [H+] * [OH–] comes closer to 1 * 10–14.
d. the solution becomes more acidic.
18. The pH of an alkaline solution is
a. less than 0.
b. less than 7.
c. more than 14.
d. more than 7.
19. Which of the following is considered neutral on the pH scale?
a. pure water
b. pure saliva
c. pure blood
d. pure urine
20. A substance that functions to prevent rapid, drastic changes in the pH of a body fluid by changing strong acids and bases into weak acids and bases is called a(n)
21. Complete the following equation:
NaHCO3 + HCl →NaCl +
22. What is the oxidation number for nitrogen in HNO3?
23. Identify the oxidizing agent and the reducing agent in the following reaction:
8NH3(g) + 6NO2(g)→7N2(g) + 12H2O(l)
a. oxidizing agent N2(g), reducing agent H2O(l)
b. oxidizing agent NH3(g), reducing agent NO2(g)
c. oxidizing agent NO2(g), reducing agent N2(g)
d. oxidizing agent NO2(g), reducing agent NH3(g)
24. Identify the oxidizing agent and the reducing agent in the following reaction:
8H+(aq) + 6Cl–(aq) + Sn(s)+ 4NO3–(aq) → SnCl62–(aq) + 4NO2(g) + 4H2O(l)
a. oxidizing agent H+(aq), reducing agent Sn(s)
b. oxidizing agent NO3–(aq), reducing agent Sn(s)
c. oxidizing agent NO3–(aq), reducing agent NO2(g)
d. oxidizing agent NO3–(aq), reducing agent H+(aq)
25. Balance the following redox reaction: Mg(s) + H2O(g)→Mg(OH)2(s) + H2(g)
a. Mg(s) + H2O(g)→ Mg(OH)2(s) + H2(g)
b. Mg(s) + 4H2O(g)→ Mg(OH)2(s) + H2(g)
c. Mg(s) + 2H2O(g)→ Mg(OH)2(s) + H2(g)
d. Mg(s) + H2O(g)→ Mg(OH)2(s) + H2(g)
26. The time required for half the atoms in a sample of a radioactive element to disintegrate is known as the element's
a. decay period.
b. life time.
c. radioactive period.
27. The half-life of a given element is 70 years. How long will it take 5.0 g of this element to be reduced to 1.25 g?
a. 70 years
b. 140 years
c. 210 years
d. 35 years
28. The elements found in carbohydrates are
a. oxygen, carbon, and hydrogen.
b. zinc, hydrogen, and iron.
c. carbon, iron, and oxygen.
d. hydrogen, iron, and carbon.
29. Steroids are classified as
b. nucleic acids.
30. The bonds between amino acids in a polypeptide are
a. glycosidic bonds.
b. ester bonds.
c. peptide bonds.
d. hydrogen bonds.
If you miss any of the answers, you can find help in the lesson shown to the right.
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