ΔΗ >0 AH2<0 H AHrxn H H† H- CI Therefore, AHrxn = [D(C-H) + D(CI–CI) – [D(C–CI) + D(H–CI) %3D [(413 kJ) + (242 kJ)] – [(328 kJ) + (431 kJ)] = (655 kJ) – (759 kJ) %3D AHrxn = -104 kJ References: Brown, T. et.al. (2012). Chemistry: The Central Science, 12th ed. Pearson Prentice Hall. Chang, R and Goldsby K. (2013). Chemistry, 11th ed. McGraw Hill. Prepared by: Bliss Capidos, RCHE 14 Name: Date Accomplished: Тopic: Write your solution/answers on your notebook. Answers will only be accepted until January 24, 2022 (Monday), 11:59 pm. 1. Write Lewis dot symbols for the following atoms and ions: (a) Te (b) I (c) P3- (d) As3+ (e) Sr2+ 2. Draw reasonable resonance structures for the following ions: (a) HSO, , (b) PO?-, (c) So?- 3. From the following data, calculate the average bond enthalpy for the N - H bond: NH3(g) NH2(g) NH(g) → NH2(g) + H(g) → NH(g) + H(g) → N(g) + H(g) AH° = 435 kJ/mol AH° = 381 kJ/mol AH° = 360 kJ/mol 4. Draw three resonance structures of sulfur dioxide (SO2). Indicate the most plausible structure(s). 5. For the reaction H2(g) + C2H4(g) C2H6(g) (a) Estimate the enthalpy of reaction, using the bond enthalpy values. (b) Calculate the enthalpy of reaction, using standard enthalpies of formation. (AH? for H2, C2H4, and C2H6 are 0 kJ/mol, 52.3 kJ/mol, and -84.7 kJ/mol, respectively.) Enthalpy (H)
ΔΗ >0 AH2<0 H AHrxn H H† H- CI Therefore, AHrxn = [D(C-H) + D(CI–CI) – [D(C–CI) + D(H–CI) %3D [(413 kJ) + (242 kJ)] – [(328 kJ) + (431 kJ)] = (655 kJ) – (759 kJ) %3D AHrxn = -104 kJ References: Brown, T. et.al. (2012). Chemistry: The Central Science, 12th ed. Pearson Prentice Hall. Chang, R and Goldsby K. (2013). Chemistry, 11th ed. McGraw Hill. Prepared by: Bliss Capidos, RCHE 14 Name: Date Accomplished: Тopic: Write your solution/answers on your notebook. Answers will only be accepted until January 24, 2022 (Monday), 11:59 pm. 1. Write Lewis dot symbols for the following atoms and ions: (a) Te (b) I (c) P3- (d) As3+ (e) Sr2+ 2. Draw reasonable resonance structures for the following ions: (a) HSO, , (b) PO?-, (c) So?- 3. From the following data, calculate the average bond enthalpy for the N - H bond: NH3(g) NH2(g) NH(g) → NH2(g) + H(g) → NH(g) + H(g) → N(g) + H(g) AH° = 435 kJ/mol AH° = 381 kJ/mol AH° = 360 kJ/mol 4. Draw three resonance structures of sulfur dioxide (SO2). Indicate the most plausible structure(s). 5. For the reaction H2(g) + C2H4(g) C2H6(g) (a) Estimate the enthalpy of reaction, using the bond enthalpy values. (b) Calculate the enthalpy of reaction, using standard enthalpies of formation. (AH? for H2, C2H4, and C2H6 are 0 kJ/mol, 52.3 kJ/mol, and -84.7 kJ/mol, respectively.) Enthalpy (H)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![AH, > 0!
AH2<0
H
AHrxn
H H† H– CI
Therefore,
AHrxn = [D(C-H) + D(CI–CI) – [D(C–CI) + D(H–CI)
%3D
= [(413 kJ) + (242 kJ)] – [(328 kJ) + (431 kJ)] = (655 kJ) – (759 kJ)
%3D
AHrxn = -104 kJ
References:
Brown, T. et.al. (2012). Chemistry: The Central Science, 12th ed. Pearson Prentice Hall.
Chang, R and Goldsby K. (2013). Chemistry, 11th ed. McGraw Hill.
Prepared by: Bliss Capidos, RCHE
14
Name:
Date Accomplished:
Тopic:
Write your solution/answers on your notebook. Answers will only be accepted
until January 24, 2022 (Monday), 11:59 pm.
1. Write Lewis dot symbols for the following atoms and ions:
(а) Те
(b) I
(c) P3-
(d) As3+
(e) Sr2+
2. Draw reasonable resonance structures for the following ions:
(a) HSO, , (b) PO?-, (c) So?-
3. From the following data, calculate the average bond enthalpy for the N - H bond:
NH3(g)
NH2(g)
NH(g)
→ NH2(g) + H(g)
→ NH(g) + H(g)
→ N(g) + H(g)
AH° = 435 kJ/mol
AH° = 381 kJ/mol
AH° = 360 kJ/mol
4. Draw three resonance structures of sulfur dioxide (SO2). Indicate the most
plausible structure(s).
5. For the reaction
H2(g) + C2H4(g)
C2H6(g)
(a) Estimate the enthalpy of reaction, using the bond enthalpy values.
(b) Calculate the enthalpy of reaction, using standard enthalpies of formation.
(AH? for H2, C2H4, and C2H6 are 0 kJ/mol, 52.3 kJ/mol, and -84.7 kJ/mol,
respectively.)
Enthalpy (H)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb326af9b-4bf0-4999-af22-39478508a610%2Fab2c7bab-bd33-4b3a-862d-dca8607617c8%2F5b604j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:AH, > 0!
AH2<0
H
AHrxn
H H† H– CI
Therefore,
AHrxn = [D(C-H) + D(CI–CI) – [D(C–CI) + D(H–CI)
%3D
= [(413 kJ) + (242 kJ)] – [(328 kJ) + (431 kJ)] = (655 kJ) – (759 kJ)
%3D
AHrxn = -104 kJ
References:
Brown, T. et.al. (2012). Chemistry: The Central Science, 12th ed. Pearson Prentice Hall.
Chang, R and Goldsby K. (2013). Chemistry, 11th ed. McGraw Hill.
Prepared by: Bliss Capidos, RCHE
14
Name:
Date Accomplished:
Тopic:
Write your solution/answers on your notebook. Answers will only be accepted
until January 24, 2022 (Monday), 11:59 pm.
1. Write Lewis dot symbols for the following atoms and ions:
(а) Те
(b) I
(c) P3-
(d) As3+
(e) Sr2+
2. Draw reasonable resonance structures for the following ions:
(a) HSO, , (b) PO?-, (c) So?-
3. From the following data, calculate the average bond enthalpy for the N - H bond:
NH3(g)
NH2(g)
NH(g)
→ NH2(g) + H(g)
→ NH(g) + H(g)
→ N(g) + H(g)
AH° = 435 kJ/mol
AH° = 381 kJ/mol
AH° = 360 kJ/mol
4. Draw three resonance structures of sulfur dioxide (SO2). Indicate the most
plausible structure(s).
5. For the reaction
H2(g) + C2H4(g)
C2H6(g)
(a) Estimate the enthalpy of reaction, using the bond enthalpy values.
(b) Calculate the enthalpy of reaction, using standard enthalpies of formation.
(AH? for H2, C2H4, and C2H6 are 0 kJ/mol, 52.3 kJ/mol, and -84.7 kJ/mol,
respectively.)
Enthalpy (H)
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