[PDF] Chem12 SM Ch05 Section5 3 final ok revised





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Section 4.1: Types of Chemical Bonds Section 4.1: Types of Chemical Bonds

Page 12. Copyright © 2012 Nelson Education Ltd. Chapter 4: Chemical Bonding 7. Answers will vary. Sample answer: Coordinate covalent bonding is like you ...



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Δ = −. Statement: The enthalpy change ΔH



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solution; an Arrhenius base forms hydroxide ions in aqueous solution. (b) A Brønsted–Lowry acid is a proton donor; a Brønsted–Lowry base is a proton.



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Chem12 SM Ch05 Section5 2 final ok revised

Chapter 5: Thermochemistry. 5.2-3. Solution: Step 1: Determine the change in temperature AT . final initial. 27.8 °C 19.8 °C.



Chem 12 SM Ch5 Review final new ok revised

(a) Answers may vary. Sample answer: Hydrogen gas has a high enthalpy of combustion releasing about 2.5 times the quantity of energy per gram than methane but 



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An enthalpy diagram of the reaction is: Page 2. Copyright © 2012 Nelson Education Ltd. Chapter 5: Thermochemistry. 5.4-2. 2. (a) Solution: Step 1: Label the 



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Chem12 SM Ch05 Section5 3 final ok revised

combustion of ethene gas to gaseous carbon dioxide and liquid water is an exothermic reaction. 3. Solution: Step 1: Use the balanced chemical equation:.

Chem12 SM Ch05 Section5 3 final ok revised

Copyright © 2012 Nelson Education Ltd. Chapter 5: Thermochemistry 5.3-1 Section 5.3: Bond Energies Tutorial 1 Practice, page 312 1. There are 3 C-H bonds and 1 C-Cl bond in chloromethane, CH3Cl(g). Given: CH

3 moln

; CH

413 kJ/molD

; CCl

1 moln

; CCl

339 kJ/molD

Required: HΔ

Analysis:

!H=n #D bonds broken

Solution: bonds broken

CHCC l

3 mol1 mol

3 mo l

HnD DD

413 kJ

mol

×1 mo l+

339 kJ

mol

1578 kJHΔ=

Statement: The energy required to separate 1 mol of chloromethane into free atoms is 1578 kJ. 2. Solution: Step 1: Write the balanced chemical equation for the combustion of 1 mol of ethene gas. C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l) Step 2: Determine the bonding of each substance by drawing structural formulas for each molecule in the reaction. Step 3: Determine the number of moles of reactants and products, the number of moles of bonds broken or formed, and the molar bond energy for each. Organize this information in a table. Substance Number of bonds per mole (nsubstance) Amount of bonds in reaction Bond energy per mole reactants C2H4 4 mol C-H bonds 1 mol C=C bonds 4 mol 1 mol 413 kJ/mol 614 kJ/mol O2 1 mol O=O bonds 3 mol 495 kJ/mol products CO2 2 mol C=O bonds 4 mol 799 kJ/mol H2O 2 mol O-H bonds 4 mol 467 kJ/mol

Copyright © 2012 Nelson Education Ltd. Chapter 5: Thermochemistry 5.3-2 Step 4: Calculate the enthalpy change, ΔH, of the reaction.

!H=n #D bonds broken $n #D bonds formed =4 mol#D C$H +1 mol#D C=C +3 mol#D O=O

4 mol#D

C=O +4 mol#D O$H =4 mol#

413 kJ

mol +1 mol#

614 kJ

mol +3 mol#

495 kJ

mol

4 mol#

799 kJ

mol +4 mol#

467 kJ

mol 0 0 =1652 kJ+614 kJ+1485 kJ$(3196 kJ+1868 kJ) !H=$1313 kJ

Statement: Since enthalpy change, ΔH, of the reaction is negative, the complete combustion of ethene gas to gaseous carbon dioxide and liquid water is an exothermic reaction. 3. Solution: Step 1: Use the balanced chemical equation: N2H2(g) + F2(g) → N2(g) + 2 HF(g) Determine the bonding of each substance by drawing structural formulas for each molecule in the reaction. Step 2: Determine the number of moles of reactants and products, the number of moles of bonds broken or formed, and the molar bond energy for each. Organize this information in a table. Substance Number of bonds per mole (nsubstance) Amount of bonds in reaction Bond energy per mole reactants N2H2 2 mol N-H bonds 1 mol N=N bonds 2 mol 1 mol 391 kJ/mol 418 kJ/mol F2 1 mol F-F bonds 1 mol 154 kJ/mol products N2 1 mol N≡N bonds 1 mol 941 kJ/mol HF 1 mol H-F bonds 2 mol 565 kJ/mol

Copyright © 2012 Nelson Education Ltd. Chapter 5: Thermochemistry 5.3-3 Step 3: Calculate the enthalpy change, ΔH, of the reaction. ()

bonds brokenbonds formed

NHNN FF

NNHF

2 mol1 mol1 mol

1 mol 2 mol

2 mo l

HnDnD DDD DD

391 kJ

mol

×1 mo l

418 kJ

mol

×1 mo l

154 kJ

mol

1 mo l

941 kJ

mol

×2 mo l

565 kJ

mol

782 kJ418 kJ154 kJ (941 kJ1130 kJ)

717 kJH

Statement: When enthalpy change, ΔH, has a negative value, there is more energy released by the formation of the bonds in the products than is absorbed by the breaking of the bonds in the reactants. Therefore, thermal energy is released to the surroundings, and the reaction is exothermic. 4. Solution: Step 1: Write the equation that represents the complete combustion of propane. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(l) Step 2: Determine the number of moles of reactants and products, the number of moles of bonds broken or formed, and the molar bond energy for each. Organize this information in a table. Substance Number of bonds per mole (nsubstance) Amount of bonds in reaction Bond energy per mole reactants C3H8 8 mol C-H bonds 2 mol C-C bonds 8 mol 2 mol 413 kJ/mol 347 kJ/mol O2 1 mol O=O bonds 5 mol 495 kJ/mol products CO2 2 mol C=O bonds 6 mol 799 kJ/mol H2O 2 mol O-H bonds 8 mol 467 kJ/mol Step 3: Calculate the enthalpy change, ΔH, of the reaction. ()

bonds brokenbonds formed

CHCC OO

COHO

8 mol2 mol5 mol

6 mol8 mol

8 mo l

HnDnD DDD DD

413 kJ

mol

×2 mo l

347 kJ

mol

×5 mo l

495 kJ

mol

6 mo l

799 kJ

mol

×8 mo l

467 kJ

mol

3304 kJ694 kJ2475 k J(4794 kJ3736 kJ)

2057 kJH

Statement: The quantity of energy released for the complete combustion of 1 mol of propane is 2057 kJ.

Copyright © 2012 Nelson Education Ltd. Chapter 5: Thermochemistry 5.3-4 Section 5.3 Questions, page 313 1. (a) Solution: Step 1: Use the balanced chemical equation to determine the bonding of each substance. H2(g) + Cl2(g) → 2 HCl(g) Step 2: Determine the number of moles of reactants and products, the number of moles of bonds broken or formed, and the molar bond energy for each. Organize this information in a table. Substance Number of bonds per mole (nsubstance) Amount of bonds in reaction Bond energy per mole reactants H2 1 mol H-H bonds 1 mol 432 kJ/mol Cl2 1 mol Cl-Cl bonds 1 mol 239 kJ/mol products HCl 1 mol H-Cl bonds 2 mol 427 kJ/mol Step 3: Calculate the enthalpy change, ΔH, of the reaction. bonds brokenbonds formed

HHCl ClHCl

1 mol1 mol2 mo l

1 mo l

HnDnD DDD

432 kJ

mol

×1 mo l

239 kJ

mol

×2 mo l

427 kJ

mol

432 kJ239 kJ854 k J

183 kJH

Statement: The ΔH for the reaction is -183 kJ. (b) Solution: Step 1: Use the balanced chemical equation to determine the bonding of each substance. N2(g) + 3H2(g) → 2 NH3(g) Step 2: Determine the number of moles of reactants and products, the number of moles of bonds broken or formed, and the molar bond energy for each. Organize this information in a table. Substance Number of bonds per mole (nsubstance) Amount of bonds in reaction Bond energy per mole reactants N2 1 mol N≡N bonds 1 mol 941 kJ/mol H2 1 mol H-H bonds 3 mol 432 kJ/mol products NH3 3 mol N-H bonds 6 mol 391 kJ/mol Step 3: Calculate the enthalpy change, ΔH, of the reaction. bonds brokenbonds formed

NNHH NH

1 mol1 mol2 mo l

1 mo l

HnDnD DDD

941 kJ

mol

×3 mo l

432 kJ

mol

×6 mo l

391 kJ

mol

941 kJ1296 kJ2346 kJ

109 kJH

Statement: The ΔH for the reaction is -109 kJ. 2. (a) Solution: Step 1: Use the balanced chemical equation to determine the bonding of each substance. HCN(g) + 2 H2(g) → CH3NH2(g)

Copyright © 2012 Nelson Education Ltd. Chapter 5: Thermochemistry 5.3-5 Step 2: Determine the number of moles of reactants and products, the number of moles of bonds broken or formed, and the molar bond energy for each. Organize this information in a table. Substance Number of bonds per mole (nsubstance) Amount of bonds in reaction Bond energy per mole reactants HCN 1 mol C-H bonds 1 mol C≡N bonds 1 mol 1 mol 413 kJ/mol 891 kJ/mol H2 1 mol H-H bonds 2 mol 432 kJ/mol products CH3NH2 1 mol C-H bonds 2 mol C-N bonds 2 mol N-H bonds 3 mol 1 mol 2 mol 413 kJ/mol 305 kJ/mol 391 kJ/mol Step 3: Calculate the enthalpy change, ΔH, of the reaction. ()

bonds brokenbonds formed

CHCN HH

CHCN NH

1 mol1 mol2 mo l

3 mol1 mol2 m ol

1 mo l

HnDnD DDD DDD

413 kJ

mol

×1 mo l

891 kJ

mol

×2 mo l

432 kJ

mol

3 mo l

413 kJ

mol

×1 mo l

305 kJ

mol

×2 mo l

391 kJ

mol

413 kJ891 kJ864 k J(1239 kJ305 kJ782 kJ)

158 kJH

Statement: The ΔH for the reaction is -158 kJ. (b) Solution: Step 1: Use the balanced chemical equation to determine the bonding of each substance. N2H4(g) + 2 F2(g) → N2(g) + 4 HF(g) Step 2: Determine the number of moles of reactants and products, the number of moles of bonds broken or formed, and the molar bond energy for each. Organize this information in a table. Substance Number of bonds per mole (nsubstance) Amount of bonds in reaction Bond energy per mole reactants N2H4 4 mol N-H bonds 1 mol N-N bonds 4 mol 1 mol 391 kJ/mol 160 kJ/mol F2 2 mol F-F bonds 2 mol 154 kJ/mol products N2 1 mol N≡N bonds 1 mol 941 kJ/mol HF 1 mol H-F bonds 4 mol 565 kJ/mol

Copyright © 2012 Nelson Education Ltd. Chapter 5: Thermochemistry 5.3-6 Step 3: Calculate the enthalpy change, ΔH, of the reaction. ()

bonds brokenbonds formed

NHNN FF

NNHF

4 mol1 mol2 mol

1 mol4 mol

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