See All test questions
Take more free SAT chemistry practice tests available from cracksat.net.
1. Two containers having 1 mole of hydrogen gas and 1 mole of oxygen gas, respectively, are opened. What will be the ratio of the rate of effusion of the hydrogen to that of the oxygen?
A. B. 4 : 1C. 8 : 1D. 16 : 1E.
2. A molecule in which the electron configuration is a resonance hybrid is
A. SO2B. C2H6C. Cl2D. HBrE. NaCl
3. What is the pH of a solution in which the [OH-] is 1.0 × 10-4?
A. -4B. +4C. +7D. -10E. +10
4. If 0.365 gram of hydrogen chloride is dissolved to make 1 liter of solution (Cl = 35.5 and H = 1.00), the pH of the solution is
A. 0.001B. 0.01C. 1D. 2E. 12
5. In the laboratory, a sample of hydrated salt was heated at 110°C for 30 minutes until all the water was driven off. The data were as follows:
Mass of the hydrate before heating = 250 grams
Mass of the hydrate after heating = 160 grams
From these data, what was the percent of water by mass in the original sample?
A. 26.5B. 36C. 47D. 56E. 90
6. Which of the following oxides dissolves in water to form an acidic solution?
A. Na2OB. CaOC. Al2O3D. ZnOE. SO3
7. In the laboratory, 20.0 milliliters of an aqueous solution of calcium hydroxide, Ca(OH)2, was used in a titration. A drop of phenolphthalein was added to it to indicate the end point. The solution turned colorless after 20.0 milliliters of a standard solution of 0.050 M HCl solution was added. What was the molarity of the Ca(OH)2?
A. 0.010 MB. 0.025 MC. 0.50 MD. 0.75 ME. 1.0 M
8. Which of the following reactions will NOT spontaneously go to completion?
A. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)B. CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(aq) + CO2(g)C. Ag+(aq) + HCl(aq) → AgCl(s) + H+(aq)D. Cu(s) + 2H+(aq) → Cu2+(aq) + H2(g); E0 = -0.34 VE. H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(aq)
9. For a laboratory experiment, a student placed sodium hydroxide crystals on a watch glass, assembled the titration equipment, and prepared a solution of 0.10 M sulfuric acid. Then he weighed 4 grams of sodium hydroxide and added it to enough water to make 1 liter of solution. What might be a source of error in the results of the titration?
A. Some sulfuric acid evaporated.B. The sulfuric acid became more concentrated.C. The NaOH solution gained weight, thus increasing its molarity.D. The NaOH crystals gained H2O weight, thus making the solution less than 0.1 M.E. The evaporation of sulfuric acid solution countered the absorption of H2O by the NaOH solution.
10. If 60. grams of NO is reacted with sufficient O2 to form NO2 that is removed during the reaction, how many grams of NO2 can be produced? (Molar masses: NO = 30. g/mol, NO2 = 46. g/mol)
A. 46.B. 60.C. 92.D. 120E. 180
11. Based on the information shown, each of the following equations represents a reaction in which the change in entropy, S, is positive EXCEPT
A. CaCO3(s) → CaO(s) + CO2(g)B. Zn(s) + 2H+(aq) → H2(g) + Zn2+(aq)C. 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g)D. NaCl(s) → Na+(aq) + Cl-(aq)E. N2(g) + 3H2(g) → 2NH3(g)
12. Cl2(g) + 2Br- (excess) → ?
When 1 mole of chlorine gas reacts completely with excess KBr solution, as shown above, the products obtained are
A. 1 mol of Cl- ions and 1 mol of Br-B. 1 mol of Cl- ions and 2 mol of Br-C. 1 mol of Cl- ions and 1 mol of Br2D. 2 mol of Cl- ions and 1 mol of Br2E. 2 mol of Cl- ions and 2 mol of Br2
13. Two water solutions are made in the laboratory, one of glucose (molar mass = 180 g/mol), the other of sucrose (molar mass = 342 g/mol). If the glucose solution had 180 grams in 1,000 grams of water and the sucrose had 342 grams in 1,000 grams of water, which statement about the freezing points of the solutions is the most accurate?
A. The glucose solution would have the lower freezing point.B. The sucrose solution would have the lower freezing point.C. The freezing point of the sucrose solution would be lowered twice as much as that of the glucose solution.D. Both solutions would have the same freezing point.E. The freezing points of the solutions would not be affected, because both solutes are nonpolar.
14. Which Ka value indicates the strongest acid?
A. 1.3 × 10-2B. 6.7 × 10-5C. 5.7 × 10-10D. 4.4 × 10-7E. 1.8 × 10-16
15. What mass of CaCO3 is needed to produce 11.2 liters of CO2 at STP when the calcium carbonate is reacted with an excess amount of hydrochloric acid? (Molar masses: CaCO3 = 100. g/mol, HCl = 36.5 g/mol, CO2 = 44.0 g/mol)
A. 25.0 gB. 44.0 gC. 50.0 gD. 100. gE. None of the above
16. By experimentation it is found that a saturated solution of BaSO4 at 25°C contains 3.9 × 10-5 mole/liter of Ba2+ ions. What is the Ksp of the BaSO4?
A. 1.5 × 10-4B. 1.5 × 10-9C. 1.5 × 10-10D. 3.9 × 10-10E. 39 × 10-9
17. What is the H° value for the decomposition of sodium chlorate, given the following information?
NaClO3 (s) → NaCl(s)+ O2 (g)
(H°f values: NaClO3(s) = -358 J/mol, NaCl(s) = -410 J/mol, O2(g) = 0 kcal/mol)
A. 52.0 JB. -52.0 JC. 768 JD. -768 JE. (768 J)
18. To the equilibrium reaction shown below:
AgCl(s) Ag+ + Cl-
a beaker of concentrated HCl (12 M) is slowly added. Which is the best description of what will occur?
A. More salt will go into solution, and the Ksp will remain the same.B. More salt will go into solution, and the Ksp will increase.C. Salt will come out of the solution, and the Ksp will remain the same.D. Salt will come out of the solution, and the Ksp will decrease.E. No change in concentration will occur, and the Ksp will increase.
19. When the following redox equation is balanced and all coefficients are reduced to lowest whole-number terms, what is the coefficient of H2O?
HCl + KMnO4 → H2O + KCl + MnCl2 + Cl2
A. 1B. 2C. 5D. 8E. 16
20. Each of the following systems is at equilibrium in a closed container. A decrease in the total volume of each container will increase the number of moles of product(s) for which system?
A. 2NH3(g) N2(g) + 3H2(g)B. H2(g) + Cl2(g) 2HCl(g)C. 2NO(g) + O2(g) 2NO2(g)D. CO(g) + H2O(g) CO2(g) + H2(g)E. Fe3O4(s) + 4H2(g) 3Fe(s) + 4H2O(g)
21. Which of the following is the correct and complete Lewis electron-dot diagram for PF3?
A. CB. CC. CD. CE. C
Hydrogen gas is collected in a eudiometer tube over water as shown above. The water level inside the tube is 40.8 millimeters higher than that outside. The barometric pressure is 730. millimeters Hg. The water vapor pressure at the room temperature of 29°C is found in a handbook to be 30.0 millimeters Hg. What is the pressure of the dry hydrogen?
A. 659.2 mm HgB. 689.2 mm HgC. 697.0 mm HgD. 740.8 mm HgE. 800.8 mm Hg
23. How many moles of electrons are required to reduce 2.93 grams of nickel ions from melted NiCl2? (Molar mass of Ni = 58.7 g/mol)
A. 0.050B. 0.10C. 1.0D. 1.5E. 2.0
* SAT is a registered trademark of the College Board, which was not involved in the production of, and does not endorse, this product.
All content of site and practice tests copyright © 2014 Max.sitemap
contactlink to us