Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Textbook Question
Chapter 8, Problem 69E
Use bond energy values (Table 3-3) to estimate ∆E for each of the following reactions in the gas phase.
a. H2 + Cl2 → 2HCl
b. N ≡ N + 3H2 → + 2NH3
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Students have asked these similar questions
2. Use the table below to estimate AH for the
reaction NO + O3 → NO2 + O2. Does this
reaction consume or produce heat?
Single Bond Energies (kJ/mol of bonds)
н сN oS F C Br I
Н 436
C 413 346
N 391 305 163
O 463 358 201 146
S 347 272
226
-
F 565 485 283 190 284 155
Cl 432 339 192 218 255 253 242
Br 366 285
201 217 249 216 193
-
I 299 213
201
278 208 175 151
-
-
Multiple Bond Energies (kJ/mol of bonds)
C=C 602
C=N 615
C=O 799
C=C 835
CEN 887
C=O 1072
N=N 418
N=O 607
N=N 945
O=O 498
The conversion of graphite into diamond is an endothermic reaction
(AH = +3 kJ mol-1).
C(graphite) → C(diamond)
1
The enthalpy change of atomisation of diamond is smaller than that of
graphite.
The bond energy of the C-C bonds in graphite is greater than that in
diamond.
2
The enthalpy change of combustion of diamond is greater than that of
graphite.
3
Which statements are correct?
A 1, 2 and 3
B 1 and 2 only C 2 and 3 only D 1 only
A student claims “C = O bonds have a larger bond energy than the other types of bonds involved in this reaction, which means they require more energy input to make.” Do you agree or disagree with the students claim? Explain your response.
Chapter 8 Solutions
Chemistry
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- Given the following data: NO2(g) NO(g) + O(g)H = 233 kJ 2O3(g) 3O2(g)H = 427 kJ NO(g) + O3(g) NO2(g) + O2(g)H = 199 kJ Calculate the bond energy for the O2 bond, that is, calculate H for: O2(g) 2O(g)H = ?arrow_forwardWrite Lewis structures for CO32, HCO3, and H2CO3. When acid is added to an aqueous solution containing carbonate or bicarbonate ions, carbon dioxide gas is formed. We generally say that carbonic acid (H2C03) is unstable. Use bond energies to estimate E for the reaction (in the gas phase) H2CO3CO2+H2O Specify a possible cause for the instability of carbonic acid.arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forward
- Explain how bond energies can be used to estimate E for a reaction. Why is this an estimate of E? How do the product bond strengths compare to the reactant bond strengths for a reaction that releases energy? A reaction that gains energy? What is the relationship between the number of bonds between two atoms and bond strength? Bond length?arrow_forwardOxygen atoms can combine with ozone to form oxygen: O3(g) + O(g) 2 O2(g) rH = 392 kJ/mol-rxn Using rH and the bond dissociation enthalpy data in Table 8.8, estimate the bond dissociation enthalpy for the oxygen-oxygen bond in ozone, O3. How does your estimate compare with the energies of an OO single bond and an O=O double bond? Does the oxygen-oxygen bond dissociation enthalpy in ozone correlate with its bond order?arrow_forwardWrite Lewis structures for CO32, HCO3, and H2CO3. When acid is added to an aqueous solution containing carbonate or bicarbonate ions, carbon dioxide gas is formed. We generally say that carbonic acid (H2CO3) is unstable. Use bond energies to estimate H for the reaction (in the gas phase) H2CO3 CO2 + H2O Specify a possible cause for the instability of carbonic acid.arrow_forward
- A commercial process for preparing ethanol (ethyl alcohol), C2H5OH, consists of passing ethylene gas. C2H4, and steam over an acid catalyst (to speed up the reaction). The gas-phase reaction is Use bond enthalpies (Table 9.5) to estimate the enthalpy change for this reaction when 37.0 g of ethyl alcohol is produced.arrow_forwardThe standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?arrow_forwardEstimate H for the following reactions using bond energies given in Table 8.5. 3CH2=CH2(g) + 3H2(g) 3CH2CH3(g) The enthalpies of formation for C6H6(g) and C6H12 (g) are 82.9 and 90.3 kJ/mol. respectively. Calculate H for the two reactions using standard enthalpies of formation from Appendix 4. Account for any differences between the results obtained from the two methods.arrow_forward
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