Full SAT Chemistry Practice Test 2: Part B

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Question 23 questions

Time 16 minutes

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1. What is the oxidation state of bromine in HBrO3?

A. –3
B. –1
C. 1
D. 3
E. 5

2. What is the percent by mass of silicon in a sample of silicon dioxide?

A. 21%
B. 33%
C. 47%
D. 54%
E. 78%

3. How many electrons does a 37Cl ion with a charge of –1 contain?

A. 16
B. 17
C. 18
D. 37
E. 38

4. CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) + 800 kJ

If 1 mole of O2(g) is consumed in the reaction given above, how much energy is produced?

A. 200 kJ
B. 400 kJ
C. 800 kJ
D. 1,200 kJ
E. 1,600 kJ

5. Which of the following is NOT true of the element sodium?

A. It takes the oxidation state +1.
B. It reacts with water to form a basic solution.
C. It forms metallic bonds in its solid uncombined form.
D. It is found in nature as a diatomic gas.
E. It reacts with a halogen to form an ionic salt.

6. What volume of a 0.200-molar solution of sodium hydroxide is required to neutralize 40 liters of a 0.300-molar hydrochloric acid solution?

A. 10 liters
B. 20 liters
C. 40 liters
D. 60 liters
E. 120 liters

7. …PH3 +…O2 →…P2O5 +…H2O

When the equation above is balanced and the coefficients are reduced to the lowest whole numbers, the coefficient for H2O is

A. 1
B. 2
C. 3
D. 4
E. 5

8. H2SO4(aq) + Ba(OH)2(aq) →

Which of the following are products of the reaction shown above?

I. O2(g)

II. H2O(l)

III. BaSO4(s)

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

9. 2Mg(s) + O2(g) → 2MgO(s)

If 48.6 grams of magnesium are placed in a container with 64 grams of oxygen gas and the reaction above proceeds to completion, what is the mass of MgO(s) produced?

A. 15.4 grams
B. 32.0 grams
C. 80.6 grams
D. 96.3 grams
E. 112 grams

10. An ideal gas in a closed inflexible container has a pressure of 6 atmospheres and a temperature of 27°C. What will be the new pressure of the gas if the temperature is decreased to –73°C?

A. 2 atm
B. 3 atm
C. 4 atm
D. 8 atm
E. 9 atm

11. Equal molar quantities of hydrogen gas and oxygen gas are present in a closed container at a constant temperature. Which of the following quantities will be the same for the two gases?

I. Partial pressure

II. Average kinetic energy

III. Average molecular velocity

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

12. Which of the following is a nonpolar molecule?

A. CO2
B. H2O
C. NH3
D. NO
E. HI

13. What is the molar concentration of a 500-milliliter solution that contains 20 grams of CaBr2 (formula weight = 200)?

A. 0.1 molar
B. 0.2 molar
C. 0.5 molar
D. 1 molar
E. 5 molar

14. The structure of BeCl2 can best be described as

A. linear
B. bent
C. trigonal
D. tetrahedral
E. square

15. 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)

Which of the following statements is true regarding the reaction given above?

A. If 1 mole of H2 is consumed, 0.5 mole of N2 is produced.
B. If 1 mole of H2 is consumed, 0.5 mole of H2O is produced.
C. If 0.5 mole of H2 is consumed, 1 mole of N2 is produced.
D. If 0.5 mole of H2 is consumed, 1 mole of NO is consumed.
E. If 0.5 mole of H2 is consumed, 1 mole of H2O is produced.

16. …Cu(s) +…NO3(aq) +…H+(aq) →…Cu2+(aq) +…NO2(g) +…H2O(l)

When the equation above is balanced with lowest whole number coefficients, the coefficient for H+(aq) will be

A. 1
B. 2
C. 3
D. 4
E. 5

17. …Cu(s) +…NO3(aq) +…H+(aq) →…Cu2+(aq) +…NO2(g) +…H2O(l)

Which of the following takes place during the reaction above?

A. Cu(s) is oxidized.
B. Cu(s) is reduced.
C. H+(aq) is oxidized.
D. H+(aq) is reduced.
E. NO3(aq) is oxidized.

18. Which of the following could be the molecular formula for a molecule with an empirical formula of CH2?

A. CH
B. CH4
C. C2H2
D. C2H6
E. C3H6

19. When CO2 is bubbled through distilled water at 25°C, which of the following is most likely to occur?

A. Solid carbon will precipitate.
B. An electrical current will be produced in an oxidation-reduction reaction.
C. The pH of the solution will be reduced.
D. The water will boil.
E. Methane (CH4) gas will be formed.

20. In which of the following processes is entropy increasing?

A. N2(g) + 3 Cl2(g) → 2 NCl3(g)
B. H2O(g) → H2O(l)
C. 2 H2O(l) → 2 H2(g) + O2(g)
D. CO(g) + 2 H2(g) → CH3OH(l)
E. 2 NO2(g) → N2O4(g)

21. Based on the phase diagram above, which series of phase changes could take place as pressure is decreased at a constant temperature?

A. Solid to liquid to gas
B. Solid to gas to liquid
C. Gas to liquid to solid
D. Gas to solid to liquid
E. Liquid to gas to solid

22. Which of the following forms of radioactive decay has (have) no electrical charge?

I. Alpha decay

II. Beta decay

III. Gamma decay

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

23. Based on the solubility products given below, which of the following salts is the most soluble?

A. BaCO3 Ksp = 5.1 × 10–9
B. PbCrO4 Ksp = 2.8 × 10–13
C. AgCl Ksp = 1.8 × 10–10
D. CaSO4 Ksp = 9.1 × 10–6
E. ZnC2O4 Ksp = 2.7 × 10–8