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a) Al(NO3)3(aq) + K3PO4(aq) → K3Al(s) + PO4(NO3)3(aq) b ..., Lecture notes of Analytical Chemistry

Putnam Career and Technical CenterAnalytical Chemistry

Write a balanced chemical equation for the reaction of aqueous solutions of aluminum nitrate and potassium phosphate. a) Al(NO3)3(aq) + K3PO4(aq) → K3Al(s) + ...

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Chem111‐2010Name:________________________
Vining‐Exam#2,Version26
1.Whichofthefollowingcompoundsaresolubleinwater:Cu(NO3)2,Al2S3,Ba3(PO4)2,andCaBr2?
a)Cu(NO3)2only
b)Cu(NO3)2andAl2S3
c)Al2S3andBa3(PO4)2
d)Ba3(PO4)2andCaBr2
e)Cu(NO3)2andCaBr2
2.AprecipitatewillformwhenaqueousNiCl2isaddedtoanaqueoussolutionof________.
a)SrI2b)Cu(NO3)2c)KOHd)Na2SO4e)NaF
3.Writeabalancedchemicalequationforthereactionofaqueoussolutionsofaluminumnitrateand
potassiumphosphate.
a)Al(NO3)3(aq)+K3PO4(aq)→K3Al(s)+PO4(NO3)3(aq)
b)3Al(NO3)2(aq)+2K3PO4(aq)→Al3(PO4)2(s)+6KNO3(aq)
c)AlNO3(aq)+KPO4(aq)→AlPO4(s)+KNO3(aq)
d)AlNO3(aq)+KPO4(aq)→AlPO4(aq)+KNO3(s)
e)Al(NO3)3(aq)+K3PO4(aq)→AlPO4(s)+3KNO3(aq)
4.Whatisthenetionicequationforthereactionofaqueoussodiumhydroxideandaqueousiron(II)chloride?
a)Na+(aq)+OH‐(aq)→NaOH(s)
b)Na+(aq)+Cl‐(aq)→NaCl(s)
c)Fe2+(aq)+2OH‐(aq)→Fe(OH)2(s)
d)Fe2+(aq)+OH‐(aq)→FeOH+(s)
e)Fe2+(aq)+2Cl‐(aq)→FeCl2(s)
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Download a) Al(NO3)3(aq) + K3PO4(aq) → K3Al(s) + PO4(NO3)3(aq) b ... and more Lecture notes Analytical Chemistry in PDF only on Docsity!

Chem 111 ‐ 2010 Name: ________________________ Vining‐ Exam #2, Version 26

  1. Which of the following compounds are soluble in water: Cu(NO 3 ) 2 , Al 2 S 3 , Ba 3 (PO 4 ) 2 , and CaBr 2? a) Cu(NO 3 ) 2 only b) Cu(NO 3 ) 2 and Al 2 S (^3) c) Al 2 S 3 and Ba 3 (PO 4 ) 2 d) Ba 3 (PO 4 ) 2 and CaBr (^2) e) Cu(NO 3 ) 2 and CaBr 2
  2. A precipitate will form when aqueous NiCl 2 is added to an aqueous solution of ________. a) SrI 2 b) Cu(NO 3 ) 2 c) KOH d) Na 2 SO 4 e) NaF
  3. Write a balanced chemical equation for the reaction of aqueous solutions of aluminum nitrate and potassium phosphate.

a) Al(NO 3 ) 3 (aq) + K 3 PO 4 (aq) → K3Al(s) + PO 4 (NO 3 ) 3 (aq)

b) 3 Al(NO 3 ) 2 (aq) + 2 K3 PO 4 (aq) → Al 3 (PO 4 ) 2 (s) + 6 KNO 3 (aq)

c) AlNO 3 (aq) + KPO 4 (aq) → AlPO 4 (s) + KNO 3 (aq)

d) AlNO 3 (aq) + KPO 4 (aq) → AlPO 4 (aq) + KNO 3 (s)

e) Al(NO 3 ) 3 (aq) + K 3 PO 4 (aq) → AlPO 4 (s) + 3 KNO 3 (aq)

  1. What is the net ionic equation for the reaction of aqueous sodium hydroxide and aqueous iron(II) chloride?

a) Na +(aq) + OH‐(aq) → NaOH(s)

b) Na

(aq) + Cl

‐

(aq) → NaCl(s)

c) Fe

2+

(aq) + 2 OH

‐

(aq) → Fe(OH) 2 (s)

d) Fe

2+

(aq) + OH

‐

(aq) → FeOH

(s)

e) Fe

2+

(aq) + 2 Cl

‐

(aq) → FeCl 2 (s)

  1. Write a balanced net ionic equation for the reaction of barium carbonate and aqueous hydrochloric acid.

a) BaCO 3 (s) + 2 H

(aq) → Ba

2+

(aq) + CO 3

2 ‐

(aq) + H 2 (g)

b) BaCO 3 (s) + 2 H+^ (aq) → Ba 2+(aq) + CO 2 (g) + H 2 O( A )

c) BaCO 3 (s) + 2 HCl(aq) → BaCl 2 (aq) + H 2 CO 3 (aq)

d) BaCO 3 (s) + 2 H +(aq) → Ba 2+(aq) + H 2 CO 3 (s)

e) BaCO 3 (s) + 2 H +(aq) → BaO(s) + CO 2 (g) + H 2 (g)

  1. Formic acid, HCO 2 H, is a weak acid. Write a net ionic equation for the reaction of aqueous formic acid and aqueous potassium hydroxide.

a) HCO 2 H(aq) + KOH(aq) → K

(aq) + HCO 2

‐

(aq) + H 2 O(A)

b) HCO 2 H(aq) + H 2 O(aq) → HCO 2

‐

(aq) + H 3 O

(A)

c) H +(aq) + OH‐(aq) → H 2 O(A)

d) HCO 2 H(aq) + OH‐(aq) → HCO 2 ‐(aq) + H 2 O( A )

e) H +(aq) + KOH(aq) → K+(aq) + H 2 O(A)

  1. What is the oxidation number of each atom in sodium phosphate, Na 3 PO 4? a) Na = +1, P = ‐3, O = ‐ 2 b) Na = +1, P = +5, O = ‐ 2 c) Na = +1, P = ‐3, O = + d) Na = ‐1, P = +5, O = ‐ 2 e) Na = 0, P = 0, O = 0
  2. All of the following are oxidation‐reduction reactions EXCEPT

a) CaCO 3 (s) → CaO(s) + CO 2 (g)

b) 2 Na(s) + Br 2 (g) → 2 NaBr(g)

c) Fe(s) + 2 HCl(aq) → FeCl 2 (aq) + H 2 (g)

d) C(s) + O 2 (g) → 2 CO(g)

e) 2 H 2 O(A) → 2 H 2 (g) + O 2 (g)

  1. If the same amount of energy in the form of heat is added to 5.00 g samples of each of the metals below, which metal will undergo the largest temperature change? Metal Specific Heat Capacity (J/g∙ o^ C) Ag 0. Al 0. Cu 0. Fe 0. Mg 1. a) Ag b) Al c) Cu d) Fe e) Mg
  2. Calculate the energy in the form of heat (in kJ) required to change 50.0 g ice at ‐15.0 °C to liquid at 65.0 °C. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific heat capacities: ice = 2.06 J/g∙ o^ C, liquid water = 4.184 J/g∙ o^ C) a) 15.5 kJ b) 16.7 kJ c) 31.8 kJ d) 128 kJ e) 145 kJ
  3. When 10.0 g KOH is dissolved in 100.0 g of water in a coffee‐cup calorimeter, the temperature rises from 25.18 °C to 47.53 °C. What is the enthalpy change per gram of KOH dissolved in the water? Assume that the solution has a specific heat capacity of 4.18 J/g∙ o^ C. a) ‐ 116 J/g b) ‐ 934 J/g c) ‐1.03 × 10 3 J/g d) ‐2.19 × 10 3 J/g e) ‐1.03 × 10 4 J/g
  4. Determine the heat of condensation of titanium(IV) chloride,

TiCl 4 (A) → TiCl 4 (g)

given the enthalpies of reaction below.

Ti(s) + 2 Cl 2 (g) → TiCl 4 (A) Δ H° = ‐804.2 kJ

Ti(s) + 2 Cl 2 (g) → TiCl 4 (g) Δ H° = ‐763.2 kJ

a) ‐1567.4 kJ b) ‐41.0 kJ c) +1.054 kJ d) +41.0 kJ e) +1567.4 kJ I also accepted (b) because the word “condensation” refers to the opposite reaction. I missed it when reversing the reaction to make the second version of the question.

  1. Which of the following chemical equations corresponds to the standard molar enthalpy of formation of SO 3?

a) SO 2 (g) + ½ O 2 (g) → SO 3 (g)

b) 2 SO 2 (g) + O 2 (g) → 2 SO 3 (g)

c) S(s) + 12 O 2 (g) → 8 SO 3 (g)

d) 2 S(s) + 3 O 2 (g) → 2 SO 3 (g)

e) S(s) + 3/2 O 2 (g) → SO 3 (g)

  1. Calculate Δ H° for the combustion of gaseous dimethyl ether,

CH 3 OCH 3 (g) + 3 O 2 (g) → 2 CO 2 (g) + 3 H 2 O(A)

using standard molar enthalpies of formation. molecule Δ Hf ° (kJ/mol) CH 3 OCH 3 (g) ‐184. CO 2 (g) ‐393. H 2 O(A)^ ‐285. a) ‐76.4 kJ b) ‐495.2 kJ c) ‐863.4 kJ d) ‐1460.3 kJ e) ‐1828.5 kJ

  1. An argon ion laser emits light at 457.9 nm. What is the frequency of this radiation? a) 4.338 × 10 ‐^19 s‐^1 b) 1.527 × 10 ‐^15 s‐^1 c) 1.373 × 10 11 s‐^1 d) 6.547 × 10 14 s‐^1 e) 2.305 × 10 18 s‐^1
  2. As the wavelength of light increases, the energy _____________ and the frequency _____________. a) increases, increases b) increases, decreases c) decreases, increases d) decreases, decreases