Full SAT Chemistry Practice Test 1: Part B

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Question 23 questions

Time 16 minutes

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1. What is the number of protons and neutrons in an atom with mass number 89 and atomic number 39?

A. 50 protons and 50 neutrons
B. 50 protons and 39 neutrons
C. 39 protons and 89 neutrons
D. 39 protons and 50 neutrons
E. 39 protons and 39 neutrons

2. …C4H10(g) +…O2(g) →…CO2(g) +…H2O(l)

When the above equation is balanced using the lowest whole-number terms, the coefficient of CO2 is

A. 2
B. 4
C. 8
D. 10
E. 13

3. Which of the following is closest in mass to a proton?

A. Alpha particle
B. Positron
C. Neutron
D. Electron
E. Hydrogen molecule

4. What is the approximate percentage composition by mass of the element oxygen in the compound HClO4?

A. 16%
B. 32%
C. 50%
D. 64%
E. 75%

5. If two atoms that differ in electronegativity combine by chemical reaction and share electrons, the bond that joins them will be

A. metallic
B. ionic
C. a hydrogen bond
D. nonpolar covalent
E. polar covalent

6. When the temperature of a 20-gram sample of water is increased from 10°C to 30°C, the heat transferred to the water is

A. 600 calories
B. 400 calories
C. 200 calories
D. 30 calories
E. 20 calories

7. What is the oxidation state of chromium, Cr, in the compound potassium dichromate, K2Cr2O7?

A. 1
B. 2
C. 3
D. 6
E. 12

8. An aqueous solution with pH 5 at 25°C has a hydroxide ion (OH) concentration of

A. 1 10–11 molar
B. 1 10–9 molar
C. 1 10–7 molar
D. 1 10–5 molar
E. 1 10–3 molar

9. 2H2O(g) → 2H2(g) + O2(g)

The volume of water vapor required to produce 44.8 liters of oxygen by the above reaction is

A. 11.2 liters
B. 22.4 liters
C. 44.8 liters
D. 89.6 liters
E. 100.0 liters

10. When 190 grams of MgCl2 are dissolved in water and the resulting solution is 500 milliliters in volume, what is the molar concentration of MgCl2 in the solution?

A. 2.0 M
B. 4.0 M
C. 8.0 M
D. 12.0 M
E. 16.0 M

11. When a fixed amount of gas has its Kelvin temperature doubled and its pressure doubled, the new volume of the gas is

A. four times greater than its original volume
B. twice its original volume
C. unchanged
D. one-half its original volume
E. one-fourth its original volume

12. In 12.4 hours, a 100 gram sample of an element decays so that its mass is 25 grams. What is the approximate half-life of this radioactive substance?

A. 1.6 hours
B. 3.1 hours
C. 6.2 hours
D. 24.8 hours
E. 49.6 hours

13. In the equation Q → + , the species represented by Q is


14. A compound with a molecular weight of 56 amu has an empirical formula of CH2. What is its molecular formula?

A. C2H2
B. C2H4
C. C4H8
D. C4H10
E. C6H12

15. The change in heat energy for a reaction is best expressed as a change in

A. enthalpy
B. absolute temperature
C. specific heat
D. entropy
E. kinetic energy

16. …NF3(g) +…H2O(g) →…HF(g) +…NO(g) +…NO2(g)

When the equation for the reaction above is balanced, how many moles of NF3 would be required to react completely with 6 moles of H2O?

A. 0.5 mole
B. 1 mole
C. 2 moles
D. 3 moles
E. 4 moles

17. Which characteristic is associated with bases?

A. React with metal to produce hydrogen gas
B. Donate an unshared electron pair
C. Always contain the hydroxide ion in their structure
D. Taste sour
E. Formed by the reaction of a nonmetal oxide and water

18. An element has the following properties: shiny, brittle, poor electrical conductivity, and high melting point. This element can be best classified as a(n)

A. alkali metal
B. halogen
C. metalloid
D. transition metal
E. noble gas

19. Which of the following forward processes produces a decrease in entropy?

I. H2O(g) → H2O(l)

II. Fe2+ (aq) + S2– (aq) → FeS(s)

III. 2SO3(g) 2SO2(g) + O2(g)

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

20. Which of the following will raise the boiling point of a sample of water?

A. Heat the water
B. Mix gasoline into the water
C. Bring the water sample to a higher altitude
D. Place the water sample on a magnetic stirrer
E. Dissolve table sugar into the water

21. Elements H and J lie in the same period. If the atoms of H are smaller than the atoms of J, then compared to atoms of J, atoms of H are most likely to

A. exist in a greater number of isotopes
B. exist in a lesser number of isotopes
C. exist in a greater number of oxidation states
D. have a greater positive charge in their nuclei
E. have a lesser positive charge in their nuclei

22. …Al(s) +…O2(g) →…Al2O3(s)

When the equation representing the reaction shown above is completed and balanced and all coefficients are reduced to lowest whole-number terms, the coefficient of O2(g) is

A. 1
B. 2
C. 3
D. 4
E. 6

23. Which of the following solids has a brilliant blue color?

A. Ca(OH)2
B. KCl
C. NaBr
D. Fe2O3
E. CuSO4