1. If If Kc=0.425 at 40.°C and Kc=0.670 at 90.°C, what is ΔH° for the reaction?...
1. If If Kc=0.425 at 40.°C and Kc=0.670 at 90.°C, what is ΔH° for the reaction?
X↽−−⇀Y
kj
2.Consider a general reaction
A(aq)⇌enzymeB(aq)
The ΔG°′ of the reaction is −7.500 kJ·mol−1. Calculate the equilibrium constant for the reaction at 25 °C.
Keq′=
What is ΔG for the reaction at body temperature (37.0 °C) if the concentration of A is 1.7 M and the concentration of B is 0.65 M?
ΔG=
3.
Attempt 9
Consider the data in the table.
| Compound | Melting point (°C) | ΔHfus (kJ/mol) | Boiling point (°C) | ΔHvap (kJ/mol) |
|---|---|---|---|---|
| HF | −83.11 | 4.577 | 19.54 | 25.18 |
| HCl | −114.3 | 1.991 | −84.9 | 17.53 |
| HBr | −86.96 | 2.406 | −67.0 | 19.27 |
| HI | −50.91 | 2.871 | −35.38 | 21.16 |
Using the data in the table, calculate ΔSfus and ΔSvap for HCl.
ΔSfus=
J/(K⋅mol)
ΔSvap=
J/(K⋅mol)
Determine the entropy change when 9.00 mol HCl(g) condenses at atmospheric pressure.
Homework Answers
Add Answer to:
1. If If Kc=0.425 at 40.°C and Kc=0.670 at 90.°C, what is
ΔH° for the reaction?...
OLLILEI UM ALLI LUUIU. Compound Melting point (°C) A Hus (kJ/mol) Boiling point (°C) AHvap (kJ/mol)...
OLLILEI UM ALLI LUUIU. Compound Melting point (°C) A Hus (kJ/mol) Boiling point (°C) AHvap (kJ/mol) HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBO -86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate AS tus and ASvap for HCL. Astus = AS = J/(K.mol) ASvap = J/(K.mol) Determine the entropy change when 5.70 mol HCI) melts at atmospheric pressure. AS = | J/K
Consider the data in the table. Compound Melting point (°C) AHus (kJ/mol Boiling point (°C) AHap...
Consider the data in the table. Compound Melting point (°C) AHus (kJ/mol Boiling point (°C) AHap (kJ/mol HF ---83.11 4.577 19.54 25.18 HC1 -114.3 1.991 -84.9 17.53 HBr -86.96 2.406 -67.0 19.27 -50.91 2.871 -35.38 21.16 Using the data in the table, calculate A Stus and AS for HBr. HI A Stus = 12.93 J/K mol) AS - 93.54 J/(K.mol) Determine the entropy change when 3.90 mol HBr(I) freezes at atmospheric pressure. as - 364.82
Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AH...
Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AH ap (kJ/mol) HF -83.11 4.577 19.54 25.18 НСІ -114.3 1.991 -84.9 17.53 HBr - 86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and ASvap for HI. ASfus = J/(K.mol) AS vap = J/(K · mol) Determine the entropy change when 6.50 mol HI(1) boils at atmospheric pressure. AS = J/K
HF Consider the data in the table. Compound Melting point (°C) AH -83.11 HCI -114.3 HBr...
HF Consider the data in the table. Compound Melting point (°C) AH -83.11 HCI -114.3 HBr -86.96 HI -50.91 4.577 (kJ/mol) Boiling point (°C) A Hvap (kJ/mol) 19.54 25.18 1.991 -84.9 17.53 2.406 -67.0 19.27 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and AS vap for HI. Astu = 12.9 J/(K.mol) ASvap = 89.0 J/(K.mol) Determine the entropy change when 3.40 mol HI(g) condenses at atmospheric pressure. рук AS = 44.0
Consider the data in the table. Compound Melting point (°C) AH (kJ/mol) Boiling point (°C) AHap...
Consider the data in the table. Compound Melting point (°C) AH (kJ/mol) Boiling point (°C) AHap (kJ/mol HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBr -86.96 -67.0 19.27 HI -50.91 -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and AS vap for HI. 2.406 A Stus = 24.1 J/(K mol) ASvap = J/(K.mol) Determine the entropy change when 7.50 mol HI(1) freezes at atmospheric pressure. AS = J/K Question Source: MRG - General...
Consider the data in the table. Compound Melting point (°C) Δ H fus (kJ/mol) Boiling point...
Consider the data in the table. Compound Melting point (°C) Δ H fus (kJ/mol) Boiling point (°C) Δ H vap (kJ/mol) HF −83.11 4.577 19.54 25.18 HCl −114.3 1.991 −84.9 17.53 HBr −86.96 2.406 −67.0 19.27 HI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ S fus and Δ S vap for HBr . Δ S fus = J / ( K ⋅ mol) Δ S v a p = J / ( K ⋅ mol)...
HF HCI HBr H86.96 83.11 - 114.3 4.577 1.991 2.406 2 871 19.54 84.9 67.0 35.38...
HF HCI HBr H86.96 83.11 - 114.3 4.577 1.991 2.406 2 871 19.54 84.9 67.0 35.38 25.18 1753 19.27 21.16 -50.91 calculate AStus and ASap for HF. Number Number As...- 24.1 J/(K- mol J/ (k mo AS 86.1 Determine the entropy change when 6,90 mol of HF(s) melts at atmospheric pressure. Number J/K Tools O Pevious @ checs Atswer O nt
Using enthalpies of formation (Appendix C), calculate ΔH ° for the following reaction at 25°C. Also...
Using enthalpies of formation
(Appendix C), calculate ΔH ° for the following reaction at 25°C.
Also calculate ΔS ° for this reaction from standard entropies at
25°C. Use these values to calculate ΔG ° for the reaction at this
temperature. COCl2(g) + H2O(l ) h CO2(g) + 2HCl(g).
Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kW/mol) 0 AG: (kJ/mol) 0 S° (J/mol-K) 20.87 ΔΗ, (kJ/mol) -946.3 - 33422 AG; {kj/mol) --859,3 -2793 (J/mol-K)...
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C....
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C. See Appendix C for data. Fe(s) + Cu2+ (aq) = Fe2+ (aq) + Cu(s) Find equilibrium constan + K at 25°C Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kJ/mol) AG; (kJ/mol (J/mol-K) 20.87 Substance or lon Ba(OH),(s) ΔΗ: (kJ/mol) -946.3 --3342.2 AG (kJ/mol) -859.3 -2793 (J/mol K) 107.1 427 Ba(OH), 8H,O(s) BaSO (8) - 1473.2 -1362.3 132.2...
OLLILEI UM ALLI LUUIU. Compound Melting point (°C) A Hus (kJ/mol) Boiling point (°C) AHvap (kJ/mol) HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBO -86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate AS tus and ASvap for HCL. Astus = AS = J/(K.mol) ASvap = J/(K.mol) Determine the entropy change when 5.70 mol HCI) melts at atmospheric pressure. AS = | J/K
Consider the data in the table. Compound Melting point (°C) AHus (kJ/mol Boiling point (°C) AHap (kJ/mol HF ---83.11 4.577 19.54 25.18 HC1 -114.3 1.991 -84.9 17.53 HBr -86.96 2.406 -67.0 19.27 -50.91 2.871 -35.38 21.16 Using the data in the table, calculate A Stus and AS for HBr. HI A Stus = 12.93 J/K mol) AS - 93.54 J/(K.mol) Determine the entropy change when 3.90 mol HBr(I) freezes at atmospheric pressure. as - 364.82
Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AH ap (kJ/mol) HF -83.11 4.577 19.54 25.18 НСІ -114.3 1.991 -84.9 17.53 HBr - 86.96 2.406 -67.0 19.27 HI -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and ASvap for HI. ASfus = J/(K.mol) AS vap = J/(K · mol) Determine the entropy change when 6.50 mol HI(1) boils at atmospheric pressure. AS = J/K
HF Consider the data in the table. Compound Melting point (°C) AH -83.11 HCI -114.3 HBr -86.96 HI -50.91 4.577 (kJ/mol) Boiling point (°C) A Hvap (kJ/mol) 19.54 25.18 1.991 -84.9 17.53 2.406 -67.0 19.27 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and AS vap for HI. Astu = 12.9 J/(K.mol) ASvap = 89.0 J/(K.mol) Determine the entropy change when 3.40 mol HI(g) condenses at atmospheric pressure. рук AS = 44.0
Consider the data in the table. Compound Melting point (°C) AH (kJ/mol) Boiling point (°C) AHap (kJ/mol HF -83.11 4.577 19.54 25.18 HCI -114.3 1.991 -84.9 17.53 HBr -86.96 -67.0 19.27 HI -50.91 -50.91 2.871 -35.38 21.16 Using the data in the table, calculate ASfus and AS vap for HI. 2.406 A Stus = 24.1 J/(K mol) ASvap = J/(K.mol) Determine the entropy change when 7.50 mol HI(1) freezes at atmospheric pressure. AS = J/K Question Source: MRG - General...
HF HCI HBr H86.96 83.11 - 114.3 4.577 1.991 2.406 2 871 19.54 84.9 67.0 35.38 25.18 1753 19.27 21.16 -50.91 calculate AStus and ASap for HF. Number Number As...- 24.1 J/(K- mol J/ (k mo AS 86.1 Determine the entropy change when 6,90 mol of HF(s) melts at atmospheric pressure. Number J/K Tools O Pevious @ checs Atswer O nt
Using enthalpies of formation
(Appendix C), calculate ΔH ° for the following reaction at 25°C.
Also calculate ΔS ° for this reaction from standard entropies at
25°C. Use these values to calculate ΔG ° for the reaction at this
temperature. COCl2(g) + H2O(l ) h CO2(g) + 2HCl(g).
Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kW/mol) 0 AG: (kJ/mol) 0 S° (J/mol-K) 20.87 ΔΗ, (kJ/mol) -946.3 - 33422 AG; {kj/mol) --859,3 -2793 (J/mol-K)...
Calculate the standard free-energy change and the equilibrium constant Kc for the following reaction at 25°C. See Appendix C for data. Fe(s) + Cu2+ (aq) = Fe2+ (aq) + Cu(s) Find equilibrium constan + K at 25°C Appendix C Thermodynamic Quantities for Substances and Ions at 25°C Substance or lon AH; (kJ/mol) AG; (kJ/mol (J/mol-K) 20.87 Substance or lon Ba(OH),(s) ΔΗ: (kJ/mol) -946.3 --3342.2 AG (kJ/mol) -859.3 -2793 (J/mol K) 107.1 427 Ba(OH), 8H,O(s) BaSO (8) - 1473.2 -1362.3 132.2...
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