Chemistry

A 140.0-g sample of water at 25.0°C is mixed with 111.7 g of a certain metal at 100,0°C

A) 0.34 J/g°C

A 32.5 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C-mol) is heated to

A) 212 g

What is the enthalpy change when 49.4 mL of 0.430 M sulfuric acid reacts with 23.3 mL of 0.309 M potassium hydroxide? H2SO4(aq)+ 2KOH(aq)-K2SO4(aq) + 2H2O() AHP-111.6 kJ/mol

A) -0.402 kJ

Two metals of equal mass with different heat. capacities are subjected to the same amount of heat . Which undergoes the smallest change in temperature?

A) The metal with the higher heat capacity.

29. Which of the following are classified as precipitation reactions?

1 AGNO3(aq)+ HCI (aq) AgCl(s) + HNO3(aq) 2 2Mg(s)+O2(g) 2MgO(s) 3. Zn(s)+ 2Ag (aq)2Ag(s)+Zn2 (aq) a. 1 only

1. Which of the following concerming electrolytes and nonelectrolytes is/are true?

1 Some molecular substances are electrolytes 2. All electrolytes are ionic substances. 3. Strong electrolytes partially ionize in solution. a. 1 only

28. Which of the following combinations will produce a precipitate?

1. AgNO3(aq) and HCI(aq) 2. HCI(aq) and NazCO3(aq) 3. NaOH(aq) and K3PO4(aq) a. 1 only

The enthalpy of fusion of ice is 6.020 kJ/mol. The heat capacity of liquid

B) 7

One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.93 liters against a constant external pressure of 1.00 atm.. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem (T-300 K; 1 L atm = 101.3 J)

B) 803 J

31. A 45.9 g sample of a metal is heated to 95.2°C and then placed in a calorimeter containing

B) Iron (c 0.45 J/g°C)

16. What is true about the value of DeltaE?

B) It is equal to zero.

What is true about the value of DeltaH?

B) It is equal to zero.

What is true about the value of w?

B) It is equal to zero.

According to the first law of thermodynamics, the energy of the universe is constant. Does this mean that AE is always equal to zero?

No, AE does not always equal zero because it refers to the system's internal energy, which is affected by heat and work.

2. Which of the following correctly describes one or more of the differences between a strong and weak electrolyte?

c.Strong electrolytes produce more ions per mole of substance in solution than weak electrolytes

75. The net ionic equation for the reaction between aqueous ammonia and hydrobromic acid is

d H (aq) + NH(aq)- NHa (aq)

173. Which of the following is/are true of gravimetric analysis?

d. 1,2, and 3

20. Which of the following would not be depicted as the individual ions on the reactant side of a complete ionic reaction?

d. CH3COOH

What minimum mass of iron (II) nitrate must be added to 10.0 of a 0.0699 Mphosphate solution in order to completely ...

e. 0.188 g

150. Calculate the molarity of a solution that contains 14.6 g of NAOH (40.0 g/mol) in 491 mL of solution.

e. 0.743 M

169. An impure sample of benzoic acid (C6HSCOOH, 122.12 g/mol) is titrated with 0.9855 M NaOH A 3.412- g sample requires 24.43 mL of titrant to reach the endpoint.

e. 86.18 %

82. Which of the following is an oxidation-reduction reaction?

e. C2H4(g)+ H2(g) -> C2Ho(g)

83. All the following are oxidation-reduction reactions except

e. Mg3N2(s)+6H2O(l) ->3Mg(OH)2(s) + 2NH3(g).

15. Which anion will form a precipitate with NH4 "?

e. none of the above

67. What is the net ionic equation for the acid-base reaction between chlorous acid and sodium hydroxide?

b. HCIO2(aq)+ OH (aq) ->CIO2 (aq) + H20(0

73. What is thenet ionic equation for the neutralization of hydrofluoric acid with sodium hydroxide?

b. HF(aq) + OH(aq)->H20(l)+ F (aq)

42. Which of the following chemical equations best represents the dissolution of a soluble group 2A metal hydroxide in water?

b. M(OH)2(s) -> M2 (ag)+ 20H (ag)

86. Which of the following reactions is an oxidation-reduction reaction?

b. NH4NO3(aq)->N20(g) + 2H20(1)

31. When a solution of lithium chloride and a solution of ammonium sulfate are mixed

b. no reaction occurs

144. How many moles of sulfate ions are there in a 0.301-L solution of 0.274 M Al2(SO4)3?

b.0.247 mol

155. What volume of 1.08 MHCI is required to prepare 182.0 mL of 0.183 M HCI?

c. 30.8 mL

121. All of the following reactions are called combination reactions except

c. Br2()+H20(I) ->HOBr(aq) + HBr(aq).

6. Which of the following aqueous solutions would be expected to be the best conductor of an electric current at room temperature?

0.10 M Na2SO4

44 Which of the following reactions best describes the dissolution of gaseous hydrogen chloride (HCI) in water?

C. HCI(g)+ HCl (g) + H2O(l) -> H3O (aq)+ CI- (aq)

46. Which of the following is not a strong acid in aqueous solution?

C. HF

In the lab, you mix two solutions (originally at the same temperature) and the temperature of

C) The chemical reaction is absorbing energy.

99. The oxidation number of carbon in the formate ion, HCOO, is

C. +2.

126. What is the balanced oxidation half-reaction provided below? Zn(s) + 2H (aq) ->Zn (aq) + H2(g)

C. Zn(s) -> Zn (aq)+ 2e-

1.A gas absorbs 0.0 J of heat and then performs 30.7 J of work. The change in internal energy of the gas is

D) -30.7 J

Which of the following statements is correct?

The system does work on the surroundings when an ideal gas expands against a constant external pressure.

23. What precipitate forms when aqueous solutions of calcium bromide and potassium phosphate are mixed?

b. Cas(PO4)2(s)

74. What is the net ionic equation for the reaction of hydrochloric acid with lithium hydroxide?

а. H (aq) + Он (аg) ->H2O (l)

94. Which of the following species cannot function as an oxidizing agent?

е O2

95. What is the oxidation number of each O in NH4(H2PO4)?

с. -2

39. Which of the following combinations will result in an acid-base reaction?

1. AgNO3(aq) and HCl(aq) 2 HCl(aq) and Na2CO3(aq) 3. NaOH(aq) and K3PO4(aq) b. 2 only

159 The concentration of Pb in a sample of wastewater is to be determined...

a. 0.0054 M

4. Which of the following solutions would be expected to be the best conductor of an electric current at room temperature?

a. 0.10 M Na2SO4

98, What is the average oxidation number of C in C6H12O6?

b. 0

56. Which of the following is a weak electrolyte in aqueous solution?

с. НзРО4

27. Which of the following concerning precipitation reactions is/are correct?

1. A precipitation reaction is a type of chemical reaction that forms a gaseous 1. product (such as CO2). 2. A precipitation reaction is possible when two or more aqueous solutions of strong or weak electrolytes are mixed 3. Only ionic compounds will react to form precipitates in a precipitation reactions. b. 2 only

38. Which of the following may be classified as an acid-base reaction?

1. AgNO3(aq)+ HCl(aq) -> AgCI(s)+ HNO3(aq) 2. 2Mg(s) + O2(g) -> 2MgO(s) 3 Zn(s)+ 2Ag (aq) -> 2Ag(s)+ Zn2 (aq) e. none

18. Which of the following concerning molecular and ionic equations is/are correct?

1. Molecular equations cannot be written for reactions involving ionic substances 2. Charge must be balanced in a properly balanced net ionic reaction. 3 In a balanced complete ionic reaction only the strong electrolytes are shown as the individual aqueous ions. e. 2 and 3

40. Which of the following concerning acid-base reactions is/are correct?

1. Only strong acids and strong bases will undergo an acid-base reaction. 2. All acid-base reactions produce water and an ionic compound (salt) as a product. 3. All reactions that form a gas are also acid-base reactions. E. None

13. Which of the following conceming electrolytes and the solubility rules is/are true?

1.The solubility rules apply only to ionic substances 2 All soluble ionic compounds are considered strong electrolytes. 3. The solubility rules apply to aqueous and non-aqueous solutions. d. 1 and 2

Consider the following processes:

2A->(1/2)B C AH 5 kJ/mol (3/2)B+ 4C 2A+ C+3D AH2-15 kJ/mol E+4A-C AH= 10 kJ/mol Calculate AH for C E+3D C) -10 kJ/mol

CH(g)+4C12(g)- CCI4(g) + 4HCI (g), AH--434 kJ Based on the above reaction, what energy change occurs when 1.2 moles of methane (CH4) reacts?

A) 5.2 x 105 J are released.

e in 2. What is the kinetic energy of a 1.56-kg object moving at 94.0 km/hr?

A) 5.32 x 102 kJ

Exactly 123.7 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C. What is the specific heat capacity of the metal?

B) 0.353 J/g°C

Consider a gas in a 1.0 L bulb at STP that is connected via a valve to another bulb that is initially evacuated. Answer the following concerning what occurs when the valve between the two bulbs is opened

B) It is equal to zero.

42 On a cold winter day, a steel metal fence post feels colder than a wooden fence post of identical size because:

B) The specific heat capacity of steel is lower than the specific heat capacity of wood.

On a cold winter day, a steel metal fence post feels colder than a wooden fence post of identical size because:

B) The specific heat capacity of steel is lower than the specific heat capacity of wood.

For a particular process q =-17 kJ and w21 kJ. Which of the following statements is false?

B) The system does work on the surroundings.

43. Which of the following reactions best describes the acid-base properties of ammonia (NH3) in aqueous solution?

C NH3(aq) + H2O(l) double reaction NH (q) +OH (aq)

26. A precipitate is expected when an aqueous solution of lithium iodide is added to an aqueous solution of a calcium nitrate.

C lead perchlorate

A fuel-air mixture is placed in a cylinder fitted with a piston. The original volume is 0.310-L When the mixture is ignited, gases are produced

C) 11.4 L

You take 295.5 g of a solid at 30.0°C and let it melt in 425 g of water. The water temperature decreases from 85.1°C

C) 331 J/g

For a particular process q 20 kJ and w 15 kJ. Which of the following statements is true?

C) AE= 35 kJ

Which of the following statements correctly describes the signs of q and w for the following exothermic process at P 1 atm and T 370 K? H2O(g) ->H20(l)

C) q is negative, w is positive.

164. In a volumetric analysis experiment, an acidic aqueous solution of methanol (CH3OH) is titrated with a solution of potassium dichromate

C. 27.6 ml

5. Which of the following solutes, dissolved in 1000 g of water, would provide the greatest number of particles?

C0.030 mol of barium chloride, BaCl2

8. Calculate the work for the expansion of CO2 from 1.0 to 4.7 liters against a pressure of 1.0 atm at constant temperature.

D) -3.7 L atm

How much heat is liberated at constant pressure when 2.35 g of potassium metal reacts with 5.68 mL of liquid iodine

D) 2.23 x 10' kJ

How much heat is required to raise the temperature of a 5.75-g sample of iron (specific heat = 0.450 J/g°C) from 25.0°C to 79.8°C?

E) 142 J

Metal Specific Heat Consider the following specific heats of metals. Zinc 0.387 J/(g°C) Magnesium 1.02 J/(g°C) Iron 0.450 J/(g°C) Silver 0.237 J/(g°C) Lead 0.127 J/(g°C)

E) Lead

81. Which of the following concening oxidation-reduction reactions is/are correct? 1. Oxidation-reduction reactions always form gaseous products. 2 At least one substance is oxidized and one substance is reduced in an oxidation- reduction reaction. 3. The species that is oxidized loses one or more electrons in an oxidation- reduction reaction.

E. 2 and 3

152. To dilute 1.00 L of a 0.600 M to 0.100 M, the final volume must be

E. 6 times the original volume

Consider the reaction: C2H5OH(l)+302(g)-> 2CO (g ) + 3H2O(l), AH=- 1.37 x 103 kJ Consider the following propositions:

I The reaction is endothermic II The reaction is exothermic. III. The enthalpy term would be different if the water formed was gaseous. Which of these propositions is (are) true? E) 1, 3

146. Which of the following solutions contains the largest number of moles of dissolved particles?

a. 25. mL of 5.0 M sodium chloride

76. Which of the following best represents the molecular equation for the reaction of aqueous ammonia with sulfuric acid?

a. 2NH3(aq)+ H2SO4(ag) (NH4)2SO4(aq)

potassium phosphate and iron(II) nitrate are mixed? 24. Which equation best represents the net ionic equation for the reaction that occurs when aqueous solutions of

a. 3Fe (aq)+2PO4 (aq) Fea(PO4)2(s)

65. What is the net ionic equation for the reaction of acetic acid, CH3COOH, with NH3?

a. CH3COOH(aq)+ NH3(aq) —> NH4 (aq) +CH3CO0 (aq)

35. What products result from mixing aqueous solutions of Cr(NO3)2(aq) and NaNO3(aq)?

a. Cr(OH)2(s) Na (aq), and NO3-(aq

68. What is the net ionic equation for the acid-base reaction that occurs when an excess of a sodium hydroxide solution is added to a solution of H2SO3?

a. H2SO3(aq) + 20H (aq) ->2H20)+ SO (ag)

64. What is the net ionic equation for the acid-base reaction that occurs when acetic acid and sodium hydroxide solutions are mixed?

a. HC2H3O2(aq) + OH (aq) ->C2H302 (aq) + H20(l)

78. What is the net ionic equation for the reaction that occurs between nitrous acid and barium hydroxide?

a. HNO2(aq)+ OH (aq)NO2 (aq)+ H2O()

87. Which of the following chemical reactions is an oxidation-reduction reaction?

a. Mg(s)+ CO2(g) -> MgO(s)+ COg)

66. What is the net ionic equation for the reaction of NH3 with HNO3?

a. NH3(aq)+ H'(aq)->NH4 (aq)

147. Which substance would produce 2 mol of particles per mole of solute when dissolved in water?

a. NH4CH3CO0

84. Which of the following chemical reactions is an oxidation-reduction reaction?

a. Zn(s) + S(s) -> ZnS(s)

122. All of the following reactions are described as decomposition reactions except

b. 2CH3OH(I) + 302(g) ->2CO2(g) + 4H20(g)

143. How many grams of lithium nitrate, LINO3 (68.9 g/mol), are required to prepare 778.4 mlL of a 0.825 M LINO3 solution?

b. 44.2 g

34. Which net ionic equation best represents the reaction that occurs when an aqueous solution of barium chloride is mixed with an aqueous solution of lithium sulfate?

b. Ba (aq)+ SO4 (aq)BaSO4(5)

91. All the following species can be reduced except

b. F

77. The net ionic equation for the reaction of nitrous acid with sodium hydroxide is

b. HNO2(aq)+ OH (aq) -> NO2 (aq)+ H20(l)

57. Which of the following is a weak electrolyte in aqueous solution?

b. NH3

115. In the following oxidation-reduction reaction, 8H (aq)+6CI (aq) + Sn(s)+ 4NO3 (aq)SnCl6 (aq)+ 4NO2(g) + 4H2O(l) what is the oxidizing agent?

b. NO3

97. In which one of the following is the oxidation number of nitrogen given incorrectly?

b. NaN3 (-1)

85. Which one of the following is necessary in order for a metal to be oxidized?

b. removal of electrons

16. Which anion will form a precipitate with Ca2?

b. ОН-

22. Identify the spectator ion(s) in the following reaction. Zn(OH)2(s)+ 2K (aq)+ 20H (aq) 2K (aq ) + Zn(OH)4 (aq)

b. к

149 What mass of H3PO4 (98.0 g/mol) is present in 86.3 L of a 0.0823 Msolution of H3PO4?

c 6.96x 102 g

All of the following are weak electrolytes in aqueous solution except

c nitric acid.

151. What volume of 0.72 M sodium bromide, NaBr, contains 6.5 x 10 mol of bromide ions?

c. 0.9 mL

145. What volume of 0.330 M Na2CO3 (106 g/mol) solution contains 32.7 of Na2CO3?

c. 0.934 L

163. In a volumetric analysis experiment, a solution of sodium oxalate (Na2C204) in acidic solution is titrated with a solution of potassium permanganate (KMnO4)

c. 19.3 mL

148 How many moles of KOH are present in 67.2 mL of 0.487 MKOH?

c. 3.27x 10-2 mol

161. Consider the reaction of HCI(aq) + NaOH(aq) NaCl(aq)+ H2O() What volume of 0.41 7 MHC is required to titrate 11.9 mL of 0.151 MNaOH?

c. 4.3 mL

41. Which of the following reactions best describes the dissolution of solid KOH(s) in water?

c. KOH(s) -> K (aq)+OH (aq)

153. What is the final concentration order of HCl in a solution prepared by addition of 922.0 mL of 4.73 M HCI to 549.0 mL of 2.03 M HCI? Assume volumes are additive.

d. 3.72 M

3. Which of the following is a nonelectrolyte in aqueous solution?

d. CH4

21, Identify the spectator ion(s) in the following reaction Cu(OH)2(s)+ 2H'(aq)+ 2CI (aq)-Cu (aq)+ 2CT(aq)+ 2H20(l)

d. Cl-

19. Which of the following would not be depicted as the individual ions on the reactant side of a complete ionic reaction?

d. CuCOs

45 Which of the following reactions best describes the acid-base properties of acetic acid (HC2H3O2) in aqueous solution?

d. HC2H3O2(aq)+ H20(l) -> H30 (aq)+ C2H3O2 (aq)

128. What is the balanced reduction half-reaction for the reaction

d. N2+6e->2N3

25. Which net ionic equation best represents the reaction that occurs when an aqueous solution of lithium nitrate is mixed with an aqueous solution of ammonium chloride?

d. No net reaction occurs

14. A student is given a sample in lab that contains one of the ions listed below. After adding a few drops of AgNO3 solution to a portion of the unknown sample, the student observed a grayish precipitate. After adding a few drops of Mg(NO3 )2 solution to another portion of the unknown sample, the student got a black precipitate. Based on these observations, what is the only possible ion in this student's sample?

d. S^2-

117. In the following reaction, 2H2O2(l) 2H2O(l)+O2(g) hydrogen peroxide functions as

d. both an oxidizing agent and a reducing agent

30. A precipitate will form when a freshly prepared aqueous carbonic acid solution is added to an aqueous solution of

d. calcium hydroxide.

90. Which of the following conversions is not an oxidation-reduction reaction?

d. conversion of CaCO3 to CaO

154. In order to dilute 71.1 mL of 0.915 M HCI to 0.100 M, the volume of water that must be added is

e 2 x 10^2 mL

An excess of sodium sulfate was added to a 1.000-L sample of polluted water. The mass of lead (II) sulfate that precipitated was 308.88 mg. Determine the mass of lead present in the sample of water.

e. 211.03 mg

116. Besides its ability to function as an acid, hydrosulfuric acid, H2S, is able to act as a reducing agent. Which one of the following equations illustrates this property of H2S?

e. 3H2S(aq)+ 2H (aq)+ 2NO3 (aq)->3S(s)+ 2NO(g) +4H20(l)

119. All of the following reactions are described as decomposition reactions except

e. NO2(g)+ H20(l)->NO(g) + 2HNO3(aq)

36. What products result from mixing aqueous solutions of Ni(C2H3O2)2(aq) and K3PO4(aq)?

e. Ni3(PO4)2(s), K (aq), and C2H3O2-(aq)

37. Which of the following is not an Arrhenius base?

e. all are Arrhenius bases