Full SAT Chemistry Practice Test 2: Part B

Test Information

Question 23 questions

Time 16 minutes

See All test questions

Take more free SAT chemistry practice tests available from cracksat.net.

1. Treatment of the dry solid with a mild oxidizing agent produces a purple solid

A. N2
B. KI
C. CCl4
D. AgNO3
E. CaCO3

2. Is the principle reaction responsible for the energy output of the sun

A. Gamma decay
B. Nuclear fusion
C. Alpha decay
D. Positron emission
E. Nuclear fission

3. Is a nuclear process that results in no change in the mass number and atomic number of a nuclide

A. Gamma decay
B. Nuclear fusion
C. Alpha decay
D. Positron emission
E. Nuclear fission

4. Responsible for most helium found on Earth

A. Gamma decay
B. Nuclear fusion
C. Alpha decay
D. Positron emission
E. Nuclear fission

5. The nuclear process that transmutes uranium-238 into thorium-234

A. Gamma decay
B. Nuclear fusion
C. Alpha decay
D. Positron emission
E. Nuclear fission

6. Has a pH of 13

A. 0.1 M MgCl2
B. 0.1 M HClO4
C. 0.1 M NH4OH
D. 0.1 M KOH
E. 0.1 M LiNO3

7. The solution with the lowest freezing point temperature

A. 0.1 M MgCl2
B. 0.1 M HClO4
C. 0.1 M NH4OH
D. 0.1 M KOH
E. 0.1 M LiNO3

8. The solution with the highest boiling point temperature

A. 0.1 M MgCl2
B. 0.1 M HClO4
C. 0.1 M NH4OH
D. 0.1 M KOH
E. 0.1 M LiNO3

9. Indicates a red flame when ionized with a Bunsen burner

A. 0.1 M MgCl2
B. 0.1 M HClO4
C. 0.1 M NH4OH
D. 0.1 M KOH
E. 0.1 M LiNO3

10. Choose the answer below that accurately describes the correct molecular shape for the molecule XeOF4.

A. Tetrahedral
B. Trigonal pyramidal
C. Trigonal bipyramidal
D. Square pyramidal
E. Flat

11. For the radioactive atom 99Tc, what is the correct number of protons and neutrons?

A. 43 protons and 56 neutrons
B. 43 protons and 99 neutrons
C. 56 protons and 43 neutrons
D. 56 protons and 99 neutrons
E. Cannot be determined

12. Which one of the following acids is NOT strong?

A. HCl
B. HBr
C. HNO3
D. H3PO4
E. H2SO4

13. Identify the equation used to determine the amount of heat required to melt 10 grams of ice.

A. Q = mCspΔT
B. Q = nΔH
C. KE = mv2
D. PE = mgh
E. PV = nRT

14. Identify the correct ground state electron configuration for Cr.

A. [Ar] 3s23d4
B. [Ar] 3s23d5
C. [Ar] 4s23d5
D. [Ar] 4s23d4
E. [Ar] 4s13d5

15. What is the hydroxide concentration for a solution with a pH of 10 at 25°C?

A. 10-14 M
B. 10-10 M
C. 10-7 M
D. 10-4 M
E. 10-1 M

16. Five hundred milliliters of solution of 0.1 M NaBr has how many milligrams of bromine?

A. 200 mg
B. 400 mg
C. 2,000 mg
D. 4,000 mg
E. 20,000 mg

17. According to the ideal gas law, what is the approximate volume that will be occupied by 0.5 mole of an ideal gas at 30°C and 3 atm pressure (gas constant R = 0.0821 L?atm/mol?K)?

A. Less than 1 L
B. 5 L
C. 10 L
D. 15 L
E. More than 20 L

18. Given that ΔG = ΔHTΔS, how is the spontaneity of an endothermic reaction expected to change with decreasing T?

A. Becomes less spontaneous
B. Becomes more spontaneous
C. Does not change
D. Decreases at first but then increases
E. Insufficient information to make a conclusion

19. Identify the element with the greatest first ionization energy.

A. Ce
B. C
C. Cl
D. Ca
E. Cs

20. Identify the molecule/ion with the greatest potential to act as a Lewis acid.

A. CH3+
B. CN
C. NH3
D. BF4
E. CO2

21. 2 Ca3(PO4)2 + 6 SiO2 + 10 C → P4 +…CaSiO3 + 10 CO

Which coefficient balances the reaction given above?

A. 2
B. 4
C. 5
D. 6
E. 8

22. A 100-milliliter solution containing AgNO3 was treated with excess NaCl to completely precipitate the silver as AgCl. If 5.7 g AgCl was obtained, what was the concentration of Ag+ in the original solution?

A. 0.03 M
B. 0.05 M
C. 0.12 M
D. 0.30 M
E. 0.40 M

23. Identify which of the following statements is FALSE.

A. The vapor pressure of a liquid decreases with increasing atmospheric pressure.
B. The value of an equilibrium constant is dependent on temperature.
C. The rate of a spontaneous reaction cannot be determined solely by its Gibbs free energy.
D. During a phase transition, the temperature of a substance must be constant.
E. The addition of a catalyst to a reaction at equilibrium has no net effect on the system.