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CHM-113 PRACTICE QUIZ 2 KEY Chapter 3 and Chapter 4

Match the reaction type with the reaction A. Combination B. Combustion D. Neutralization E. Precipitation

C. Decomposition F. Single-displacement

1. 2. 3. 4. 1. D

Ba(OH)2 + H2SO4  2 H2O + BaSO4 Cl2 + 2 NaI  2NaCl + I2 P4 + 10 Cl2  4 PCl5 H2O2  H2 + O2 2. F 3. A 4. C

5.

Select the correct statement below that fits a theoretical yield when a reaction between equal masses of Ca and O occurs to produce CaO. A. B. C. D. E.

6.

Using the image, select the chemical equation that best represents the balanced chemical reaction (using smallest whole number coefficients). A. B. C. D. E.

7.

The mass of CaO produced equals the sum of the starting masses of Ca and O The mass of CaO produced is more than the sum of the masses of Ca and O The mass of CaO produced is less than the sum of the masses of Ca and O There is not enough information to complete this question None of the answer choices are correct

X2 + YX  YX2 2 X2 + 4 YX  4 YX2 X2 + 2 YX  2 YX2 Y2 + YX  Y2X None of the above

Select the correct set of coefficients for the balanced chemical reaction using smallest whole number coefficients. RbOH(aq) + Al2(SO4)3(aq)  Rb2SO4(aq) + Al(OH)3(s) A. B. C. D. E.

1, 1, 1, 1 3, 1, 2, 2 3, 1, 3, 1 6, 1, 3, 2 12, 1, 12, 6

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Revised 8/18/19

8.

Which of the following equations is not balanced?

A. B. C. D. E.

9.

When C4H8O4, tetrose, dissolves in water A. B. C. D. E.

10.

each of the Na, S, and O atoms is surrounded by water. each of the Na+ and SO42- ions is surrounded by water. each Na atom and SO4 molecule is surrounded by water. each Na2SO4 unit is surrounded by water. each Na+, S2-, and O2- ion is surrounded by water.

What precipitate(s) form when mixing aqueous solutions of Ca2+, Cl-, CO32-, and NO3-. A. B. C. D. E.

12.

each C4+, H+, and O2- ion is surrounded by water each CH and OH- particles are surrounded by water each CH and OH particles are surrounded by water each C4H8O4 molecule is surrounded by water tetrose does not dissolve in water

When Na2SO4(s) dissolves in water, A. B. C. D. E.

11.

C6H12O6 + 6 O2  6 CO2 + 6 H2O C2H5OH(l) + 3 O2(g)  2 CO2(g) + 2 H2O(g) C2H4(g) + 3 O2(g)  2 CO2(g) + 2 H2O(g) C3H8(l) + 5 O2(g)  3 CO2(g) + 4 H2O(g) C3H6O(l) + 4 O2(g)  3 CO2(g) + 3 H2O(g)

CaCO3 CaCO3 and CaCl2 Ca(NO3)2, CaCO3, and CaCl2 Ca(NO3)2 and CaCl2 No precipitates will form

Which of the following is least soluble in water? A. B. C. D. E.

K2CO3 KHCO3 Ca(HCO3)2 CaCO3 KNO3

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Revised 8/18/19

13.

When dilute HCl is added to a solution, a white precipitate forms. Which ion was likely in the solution? A. B. C. D. E.

14.

Which solution will produce a precipitate when mixed with a solution of Ba(NO3)2? A. B. C. D. E.

15.

16.

Ag+ Cu2+ Na+ Ca2+ Sr2+

CuCl2(aq) NaCH3CO2(aq) NaCl(aq) NH4I(aq) (NH4)2SO4(aq)

Select the correct statements below. I. II. III. IV.

Table salt is a good conductor of electricity because it is a strong electrolyte Table sugar is a weak conductor of electricity because it is a weak electrolyte Methanol, CH3OH, cannot conduct electricity but LiOH can. Acetic acid is a better conductor of electricity than chloric acid.

A. B. C. D. E.

I only I, III, and IV only I and III only IIII and IV only I, II, IV only

Which of the following is incorrectly paired? A. B. C. D. E.

H2SO4; strong acid NaOH; strong electrolyte H3PO4; weak acid HClO4; weak electrolyte All of the above are correctly paired

17.

When a solution of magnesium nitrate is mixed with a solution of sodium phosphate, the solid that forms is magnesium phosphate. Select the equation that represents the complete ionic equation.

A. B. C. D. E.

Mg(NO3)2(aq) + Na2PO4(aq)  MgPO4(s) + NaNO3(aq) Mg2+(aq) + PO43-(aq)  MgPO4(s) 3Mg(NO3)2(aq) + 2Na3PO4(aq)  Mg3(PO4)2(s) + 6NaNO3(aq) 3Mg2+(aq) + 2PO43-(aq)  Mg3(PO4)2(s) 3Mg2+(aq)+6NO3-(aq) + 6Na+(aq) + 2PO43-(aq) Mg3(PO4)2(s)+6NO3-(aq)+ 6Na+(aq)

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Revised 8/18/19

18.

When a solution of magnesium nitrate is mixed with a solution of sodium phosphate, the solid that forms is magnesium phosphate. Select the equation that represents the net ionic equation.

A. B. C. D. E.

Mg(NO3)2(aq) + Na2PO4(aq)  MgPO4(s) + NaNO3(aq) Mg2+(aq) + PO43-(aq)  MgPO4(s) 3Mg(NO3)2(aq) + 2Na3PO4(aq)  Mg3(PO4)2(s) + 6NaNO3(aq) 3Mg2+(aq) + 2PO43-(aq)  Mg3(PO4)2(s) 3Mg2+(aq)+6NO3-(aq) + 6Na+(aq) + 2PO43-(aq) Mg3(PO4)2(s)+6NO3-(aq)+ 6Na+(aq)

19.

Which of the following atoms has an oxidation number of +6 in H2SO4? A. B. C. D. E.

20.

What is the oxidation number of Cr in Cu2CrO4? A. B. C. D. E.

21.

H S O Both S and O None of the atoms

+12 +3 +4 +5 +6

Select the correct statements. I. II. III. IV.

Reduction is the loss of electrons, and oxidation is the gain of electrons Reduction is the gain of electrons, and oxidation is the loss of electrons The reactant that is reduced is also called the reducing agent, and the reactant that is oxidized is called the oxidizing agent. The reactant that is oxidized is also called the reducing agent, and the reactant that

V.

is reduced is called the oxidizing agent. The sum of all the oxidation numbers in a compound is equal to the charge of that compound.

A. B. C. D. E.

I and III only II and IV only I, III, and V only II, IV, and V only V only

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Revised 8/18/19

22.

In the following reaction: A. B. C. D. E.

23.

24.

B. C. D. E.

PbO is the reducing agent and O2 is the oxidizing agent PbO is the reducing agent and PbO2 is the oxidizing agent O2 is the reducing agent and PbO is the oxidizing agent PbO2 is the reducing agent and PbO is the oxidizing agent None of the above

The percent composition (by mass) is the same for each element in that compounds empirical and molecular formulas. Three different compounds having the same percent composition and the same molar mass will also have the same empirical formula. An element with the largest atomic mass is always the element present in the highest percentage by mass in a compound. A and B are correct A, B, and C are correct

What is the percent by mass of carbon in acetone, C3H6O? A. B. C. D. E.

26.

2 PbO(s) + O2(g)  2 PbO2(s)

Select the correct statement below. A.

25.

CH4 is oxidized and HCl is reduced CH4 is oxidized and is Cl2 reduced CHCl3 is oxidized and HCl is reduced Cl2 is oxidized and CH4 is reduced None of the above

In the following reaction: A. B. C. D. E.

CH4 + 3Cl2  CHCl3 + 3HCl

1.60 % 30.0 % 62.0 % 20.7 % 50.0 %

What is the percent by mass of oxygen in Ca(OH)2? A. B. C. D. E.

40.0 % 33.3 % 36.3 % 43.2 % 28.0 %

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Revised 8/18/19

27.

Select the correctly paired empirical and molecular formulas Molecular Empirical A. C3H2 CH B. C6H2 C2H C. C3H2OH C3H2OH D. C6H12 C2H4 E. C4H8 C2H4

28.

What is the empirical formula of a compound that is 3.05% carbon, 0.26% hydrogen, and 96.69% iodine? A. B. C. D. E.

29.

A compound has an empirical formula of C2H2O. If the experimental molecular weight is found to be ~170 g/mol, the molecular formula of the compound is: A. B. C. D. E.

30.

113.19 g/mol 124.21 g/mol 141.39 g/mol 132.17 g/mol 114.05 g/mol

How many atoms of hydrogen are in ONE molecule of (NH4)2SO4? A. C. D. E.

32.

C3H6O3 C2H2O C4H4O2 C6H6O3 C8H8O4

What is the molar mass of (NH4)2SO4? A. B. C. D. E.

31.

C2HI7 CH2I5 C3H2I11 CHI3 CHI

4 6 1 8

B.

2

How many moles are there in 8.5 x 1025 molecules of CO2? A. B. C. D.

1.4 X 102 mol 7.1 X 10-2 mol 5.1 X 1049 mol 8.5 X 1025 mol

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E. 33.

How many hydrogen atoms are in 4 molecules of isopropyl alcohol, C3H7O? A. B. C. D. E.

34.

3.31 x 1023 atoms of C 1.65 atoms of C 3 atoms of C 9.94 x 1023 atoms of C 189 atoms of C

The products of a combustion reaction are shown in the diagram in the exact quantities after a chemical reaction of a hydrocarbon with oxygen. Determine the chemical formula of the hydrocarbon reactant. A. B. C. D. E.

36.

2.4 x 1023 atoms of H 4 atoms of H 28 atoms of H 1.7 x 1025 atoms of H 7 atoms of H

How many carbon atoms are in 0.550 mol of isopropyl alcohol (C3H7O)? A. B. C. D. E.

35.

4.3 x 1025 mol

CH4 C2H6 C4H10 C6H12O6 C5H12

In a chemical reaction, 3 moles of hydrogen are reacted with 1 mole of nitrogen. Which of the following boxes best represents the product that is produced.

A A. B. C. D. E.

B

C

D

Box A Box B Box C Box D None of the boxes

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Revised 8/18/19

37.

Bath salts such as Epsom contain hydrate salts such as MgSO4·7H2O (magnesium sulfate heptahydrate). When heated, water is released as vapor and anhydrous MgSO4 remains. Determine how many moles of vapor are released when 15.5 g of MgSO4·7H2O are heated. Hint: Include H2O when calculating the molar mass. A. B. C. D. E.

38.

0.291 mol 0.142 mol 0.253 mol 0.0629 mol 0.129 mol

The image below represents the reactants used to produce ammonia. Determine how many moles of hydrogen are required to produce 13.0 mol of the product. You must first determine the balanced chemical reaction – the amounts in the image are not exact.

A. B. C. D. E.

4.00 mol 10.0 mol 39.0 mol 6.50 mol 19.5 mol

39.

What is the total mass, in grams, of products when 2.20 g of propane is burned in excess oxygen according to the balanced chemical reaction below? C3H8 + 5O2  3CO2 + 4H2O A. 2.20 g B. 3.60 g C. 6.60 g D. 10.2 g E. 44.1 g

40.

What is the maximum amount of Al2Cl6 that can be formed from the reaction of 4.0 mol of Al with 5.0 mol of Cl2 according to this equation? 2 Al(s) + 3 Cl2(g)  Al2Cl6(s) A. 9.0 mol B. 3.7 mol C. 2.0 mol D. 1.7 mol E. 5.2 mol

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Revised 8/18/19

41.

The image below shows the reaction between hydrogen and chlorine gas. Based on the starting amounts provided for the reactants, select the true statement below. A. B. C. D. E.

42.

43.

Cl2 is the limiting reactant because it is present in the lesser amount Cl2 is the limiting reactant because it is completely consumed during the reaction H2 is the limiting reactant because it is present in excess after th reaction H2 is the limiting reactant because it is present in a lesser amount None of the statements are true.

Aspirin (C9H8O4) may be synthesized by mixing salicylic acid (C7H6O3) with excess acetic anhydride (C4H6O3). When 2.0 g of salicylic acid is mixed with excess acetic anhydride, 1.7 g of aspirin is collected. What is the percent yield of this reaction? The balanced equation is

C7H6O3 + C4H6O3  C9H8O4 + C2H4O2

A. C. E.

B. D.

98 % 77 % 55 %

85 % 65 %

A student reacts 6.0 g solid sulfur and 5.0 g oxygen gas at 95% efficiency to produce sulfur trioxide according to the chemical reaction below. What was the student’s actual yield? S8 (s) + 12 O2 (g)  8 SO3 (g) A. C. E.

44.

7.9 g 14 g 11 g

B. D.

8.3 g 15 g

How many grams are required to create 350. mL of a 1.42 M NaCl solution? A. B. C. D. E.

237 g 0.237 g 8.50 x 10-3 g 5.99 g 29.0 g

1.42 mol NaCl | 0.350 L | 58.44 g NaCl 1 L NaCl | | 1 mol NaCl Copyright ©2019 Grand Canyon University

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45.

What volume of 3.0 M NaOH can be prepared using exactly 96.0 g of NaOH? A. C. E.

46.

B. D.

0.70 L 1.25 L

What is the concentration of Na2SO4 in a solution if the concentration of Na+ ions is 0.35 M?

A. C. E. 47.

0.14 L 0.80 L 7.20 L

0.35 M 0.12 M 0.70 M

B. D.

0. 18 M 1.1 M

A solution with a total volume of 750. mL contains 37.1 g Mg(NO3)2. Determine the concentration of nitrate ions in solution. A. C. E.

0.667 M 6.67 x 10-4 M 98.9 M

B. D.

0.334 M 3.34 x 10-4 M

37.1 g Mg(NO3)2 | 1 mol Mg(NO3)2 | 2 mol NO3- | 148.3 g Mg(NO3)2 |1 mol Mg(NO3)2 | 0.750 L 48.

A student removes 25 mL of 3.0 M NaOH and dilutes it to final volume of 350 mL. What is the concentration of the resulting solution.? A. C. E.

49.

B. D.

0.024 M 0.10 M

What volume of 17.4 M HCl should be used to prepare 500. mL of a 6.00 M solution of HCl? A. C. E.

50.

42 M 75 M 0.21 M

1450 mL 0.209 mL 2.9 mL

B. D.

209 mL 172 mL

What volume of water must be added to 300 mL of 0.75 M HCl to dilute the solution to 0.25 M? A. C. E.

900 mL 300 mL 100 mL

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B. D

600 mL .930 mL

Revised 8/18/19...