LL ORG CHEM
6th Edition
ISBN: 9781264840083
Author: SMITH
Publisher: MCG
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Textbook Question
Chapter 6, Problem 44P
Consider the following reaction:
a. Use curved arrows to show the movement of electrons.
b. Calculate
c. Draw an energy diagram assuming that
d. What is
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5.
Calculate AH for the following reaction.
C6H6(1) + 02 (g) --
---→ C(s) + H20(1)
State whether the reaction is exothermic or endothermic and why. The molar enthalpies of combustion
of carbon, water and benzene, are -394 kJ/mol, -286 kJ/mol, and -3,267.4 kJ/mol, respectively.
[4A,2T]
I
7. Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. Be sure to
show a lewis structure for each molecule.
CH, (g) + 20, (g)
·CO, (g) + H,O (g)
Bond Bond Enthalpy
(kJ/mol)
C-O
351
C=0
799
CEO
1070
O-O
142
O=0
498
C-H
414
O-H
460
Calculate AH for the reaction:
2NH3 (g) + O2(g) → N2H4 (1) + H2O(1)
given the following data:
2NH3 (g) + 3N20(g) → 4N2(g) + 3H2O(1) AH = –1010. kJ
N20(g) + 3H2 (9) → N¿H4(1)+H2O(1) AH = -317 kJ
N2H4 (1) + O2 (g) → N2(g)+ 2H2O(1)
AH = -623 kJ
H2 (9) + 02 (9) → H2O(1)
AH = -286 kJ
ΔΗ -
kJ
Chapter 6 Solutions
LL ORG CHEM
Ch. 6.2 - Prob. 2PCh. 6.3 - Problem 6.3 By taking into account...Ch. 6.3 - Problem 6.4 Use curved arrows to show the movement...Ch. 6.3 - Problem 6.5 Follow the curved arrows and draw the...Ch. 6.4 - Prob. 6PCh. 6.4 - Problem 6.7 Use the values in Table 6.2 to...Ch. 6.4 - Prob. 8PCh. 6.5 - aWhich Keq corresponds to a negative value of G,...Ch. 6.5 - Given each of the following values, is the...Ch. 6.5 - Given each of the following values, is the...
Ch. 6.5 - The equilibrium constant for the conversion of the...Ch. 6.6 - Prob. 13PCh. 6.6 - For a reaction with H=40kJ/mol, decide which of...Ch. 6.6 - For a reaction with H=20kJ/mol, decide which of...Ch. 6.7 - Draw an energy diagram for a reaction in which the...Ch. 6.7 - Prob. 17PCh. 6.7 - Prob. 18PCh. 6.8 - Problem 6.19 Consider the following energy...Ch. 6.8 - Draw an energy diagram for a two-step reaction,...Ch. 6.9 - Which value if any corresponds to a faster...Ch. 6.9 - Prob. 22PCh. 6.9 - Problem 6.23 For each rate equation, what effect...Ch. 6.9 - Prob. 24PCh. 6.10 - Identify the catalyst in each equation. a....Ch. 6 - Draw the products of homolysis or heterolysis of...Ch. 6 - Explain why the bond dissociation energy for bond...Ch. 6 - Classify each transformation as substitution,...Ch. 6 - Prob. 29PCh. 6 - 6.31 (a) Add curved arrows for each step to show...Ch. 6 - Prob. 35PCh. 6 - 6.39. a. Which value corresponds to a negative...Ch. 6 - Prob. 40PCh. 6 - For which of the following reaction is S a...Ch. 6 - Prob. 42PCh. 6 - Prob. 43PCh. 6 - 6.44 Consider the following reaction: .
Use curved...Ch. 6 - Prob. 45PCh. 6 - 6.50 The conversion of acetyl chloride to methyl...Ch. 6 - Prob. 50PCh. 6 - Prob. 53P
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- Calculate the enthalpy change when 1.0(1 g of methane is burned in excess oxygen according to the reaction CH,(g) 4- 2O2(g) ->CO2(g) + H-CH/) 1H = -891 kJ/molarrow_forwardn Fig. 10.1, what kind of energy does ball A possess initially when at rest at the top of the hill? What kind of energies are involved as ball A moves down the hill? What kind of energy does ball A possess when it reaches the bottom of the hill and stops moving after hitting ball B? Where did the energy gained by ball B, allowing it to move up the hill, come from?arrow_forwardUsing the BDE values from Appendix 3, calculate the Hrxn0 value and state if the reaction below is exothermic or endothermic. CH2=CH2 + HCl CH3CH2Clarrow_forward
- Which statement best describes the energy change for the reaction associated with this energy diagram? products reactants Reaction Progress O This is an exothermic reaction with AH 0 This is an endothermic reaction with AH > 0 O This is an exothermic reaction with AH > 0 This is an endothermic reaction with AH < 0 Energyarrow_forwardUsing bond energies from the table, estimate ΔH for the reaction below. The OH group on the product side is attached to a carbon.CH2=CH2(g) + H2O(g) ↔ CH3CH2OH(g) Bond Energies, kJ/mol Single Bonds H C N O S F Cl Br I H 432 C 411 346 N 386 305 167 O 459 358 201 142 S 363 272 --- --- 286 F 565 485 283 190 284 155 Cl 428 327 313 218 255 249 240 Br 362 285 243 201 217 249 216 190 I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 CºC 835 CºN 887 CºO 1072 N=N 418 N=O 607 S=O (in SO2) 532 NºN 942 O2 494 S=O (in SO3) 469arrow_forward1. Using two or more of the following. N.(g) + 10,(g) → N.O.(s); AH = 83.7 kJ N.(g) + O(g) → 2NO(g): AH 180.4 kJ IN.(g) + O.(g) → NO.(g): AH = 33.2 KJ IN.(g) + H₂(g) → NH,(g); AH = -45.9 kJ determine AH" for the following reaction. NO(g) + NO₂(g) → N₂O(g)arrow_forward
- Calculate ΔH° for each reaction. a. HO• + CH4 → •CH3 + H2O b. CH3OH + HBr → CH3Br + H2Oarrow_forwardIt is interesting to compare the “fuel value” of a hydrocarbonin a hypothetical world where oxygen is not thecombustion agent. The enthalpy of formation of CF4(g) is-679.9 kJ/mol. Which of the following two reactions is themore exothermic?CH4(g) + 2 O2(g) ----->CO2(g) + 2 H2O(g)CH4(g) + 4 F2(g) ------> CF4(g) + 4 HF(g)arrow_forwardConsider methane, CH₄, and hydrogen, H₂, as possible fuel sources a. Write the chemical equation for the complete combustion of each fuel. Then find the enthalpy of combustion, △Hcomb, of each fuel. Express your answers in kJ/mol and kJ/g. Assume that water vapour, rather than liquid water, is formed in both reactions. b. Which is the more energetic fuel, per unit mass? c. Consider a fixed mass of each fuel. Which fuel would allow you to drive a greater distance? Explain briefly d. Describe how methane and hydrogen could be obtained. Which of these methods do you think is less expensive? Explain. e. Which fuel do you think is more environmentally friendly? Explain.arrow_forward
- In reaction 1, If we had used 4 grams of NAOH instead of 2 g, would the heat gained by the solution [#6] have been larger, smaller or the same? Briefly explain.arrow_forwardCH,(9) + 2 O,(g) AH = -809.0 kJ/mol rxn Co,(9) + 2 H,0(g) ΔΗ. = -81.3 kJ 'cond 2 H,0U) Given the energy diagram above, what is AH when two moles of methane are combusted? -401.15 kJ +1604.6 kJ -802.3 kJ +802.3 kJ +401.15 kJ O -1604.6 kJarrow_forwardCalculate ΔH° for the reaction using the given bond dissociation energies. CH4(g)+2O2(g)⟶CO2(g)+2H2O(g) Bond ΔH° (kJ/mol) O–OO–O 142 H–OH–O 459 C−HC−H 411 C=OC=O 799 O=OO=O 498 C–OC–O 358 What type of reaction is this?arrow_forward
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