SAT Chemistry Online Practice Test 1: Part B

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Question 24 questions

Time 16 minutes

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1. Question below refers to the following pairs of substances:

Are strong electrolytes in aqueous solutions

A. NH3 and N2H4
B. 16O and 17O
C. NH4Cl and NH4NO3
D. CH3OCH3 and CH3CH2OH
E. O2 and O3

2. Two immiscible liquids, when shaken together vigorously, may form

A. a solution
B. a tincture
C. a sediment
D. a hydrated solution
E. a colloidal dispersion

3.

A thermometer is used to record the cooling of a confined pure substance over a period of time. During which interval on the cooling graph above is the system undergoing a change of state from a liquid to a solid?

A.
B.
C.
D.
E.

4. If a principal energy level of an atom in the ground state contains 18 electrons, they will be arranged in orbitals according to the pattern

A. s6p6d6
B. s2p6d10
C. s2d 6f10
D. s2p6f10
E. s2p2f14

5. Which of the following molecules is a saturated hydrocarbon?

A. C3H8
B. C2H4
C. C4H6
D. CH3OH
E. CH3COOH

6. A liter of hydrogen is at 5.0°C temperature and under 640. torr pressure. If the temperature were raised to 60.0°C and the pressure decreased to 320. torr, how would the liter volume be modified?

A. C
B. C
C. C
D. C
E. C

7. Of the following statements about the number of subatomic particles in an ion of , which is (are) true?

I. 16 protons

II. 14 neutrons

III. 18 electrons

A. II only
B. III only
C. I and II only
D. I and III only
E. I, II, and III

8. The most active metallic elements are found in

A. the upper right corner of the periodic chart
B. the lower right corner of the periodic chart
C. the upper left corner of the periodic chart
D. the lower left corner of the periodic chart
E. the middle of the periodic chart, just beyond the transition elements

9. If 1 mole of each of the following substances was dissolved in 1,000 grams of water, which solution would have the highest boiling point?

A. NaCl
B. KCl
C. CaCl2
D. C6H10O5
E. C12H22O11

10. A tetrahedral molecule, XY4, would be formed if X were using the orbital hybridization

A. p2
B. s 2
C. sp
D. sp 2
E. sp 3

11. In the following reaction, how many liters of SO2 at STP will result from the complete burning of pure sulfur in 8 liters of oxygen?

S(s) + O2 (g)→SO2 (g)

A. 1
B. 4
C. 8
D. 16
E. 32

12.

In the above laboratory setup to measure the pressure of the confined gas, what will be true concerning the calculated pressure on the gas?

A. The gas pressure will be the same as the atmospheric pressure.
B. The gas pressure will be less than the atmospheric pressure.
C. The gas pressure will be greater than the atmospheric pressure.
D. The difference in the height (h) of mercury levels is equal to the pressure of the gas.
E. The height (h) of mercury has no effect on the pressure calculation since the column of mercury is only used to enclose the gas volume.

13. Which of the following changes in the experiment shown in question 12 would cause the pressure in the glass container to vary from that shown?

A. Use a U-tube of a greater diameter and maintain the height of mercury.
B. Increase the temperature of gas in the tube.
C. Increase the length of the upper portion of the right side of tubing.
D. Use a U-tube of a smaller diameter and maintain the height of mercury.
E. Replace the flask with one that has the same volume but has a flat bottom.

14. Which of the following can be classified as amphoteric?

A. Na3PO4
B. HCl
C. NaOH
D. HSO4-
E. C2O42-

15. Standard conditions (STP) are

A. 0°C and 2 atm
B. 32°F and 76 torr
C. 273 K and 760 mm Hg
D. 4°C and 7.6 cm Hg
E. 0 K and 760 mm Hg

16. Laboratory results showed the composition of a compound to be 58.81% barium, 13.73% sulfur, and 27.46% oxygen. What is the empirical formula of the compound?

A. BaSO4
B. BaS2O
C. Ba2SO3
D. BaS2O4
E. Ba2SO4

17. What is the percentage composition of calcium in calcium hydroxide, Ca(OH)2? (1 mol = 74 g)

A. 40%
B. 43%
C. 54%
D. 69%
E. 74%

18. How many grams of hydrogen gas can be produced from the following reaction if 65 grams of zinc and 65 grams of HCl are present in the reaction?

Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)

A. 1.0
B. 1.8
C. 3.6
D. 7.0
E. 58

19. The following statements were recorded while preparing carbon dioxide gas in the laboratory. Which one involves an interpretation of the data rather than an observation?

A. No liquid was transfered from the reaction bottle to the beaker.
B. The quantity of solid minerals decreased.
C. The cloudiness in the last bottle of limewater was caused by the product of the reaction of the colorless gas and the limewater.
D. The bubbles of gas rising from the mineral remained colorless throughout the experiment.
E. There was a 4°C rise in temperature in the reaction vessel during the experiment.

20.

The above laboratory setup can be used to prepare which of the following?

I. CO2(g)

II. H2(g)

III. O2(g)

A. I only
B. III only
C. I and III only
D. II and III only
E. I, II, and III

21.

The missing product in the nuclear reaction represented above is

A.
B.
C.
D.
E.

22.

Which of the following is (are) true regarding the aqueous dissociation of HCN, Ka = 4.9 × 10-10, at 25°C?

I. At equilibrium, [H+] = [CN-].

II. At equilibrium, [H+] > [CN-].

III. HCN(aq) is a strong acid.

A. I only
B. II only
C. I and II only
D. I and III only
E. I, II, and III

23. This question pertains to the reaction represented by the following equation:

2NO(g)+ O2 (g) 2NO2 (g)+ 150 kJ

Suppose that 0.8 mole of NO is converted to NO2 in the above reaction. What amount of heat will be evolved?

A. 30 kJ
B. 60 kJ
C. 80 kJ
D. 130 kJ
E. 150 kJ

24. How does a Brønsted-Lowry acid differ from its conjugate base?

A. The acid has one more proton.
B. The acid has one less proton.
C. The acid has one more electron.
D. The acid has one less electron.
E. The acid has more than one additional proton.