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일반화학/[19장] 화학 열역학63

ΔG 계산. Cu|Cu2^+(0.0200 M)||Ag^+(0.0200 M)|Ag ΔG 계산. Cu|Cu2^+(0.0200 M)||Ag^+(0.0200 M)|Ag 다음 셀의 열역학 퍼텐셜과 셀 반응과 관련된 자유 에너지 변화를 계산하시오. Cu | Cu2^+ (0.0200 M) || Ag^+ (0.0200 M) | Ag > Ag^+ + e^- → Ag(s) ... E° = +0.799 V > Cu^2+ + 2e^- → Cu(s) ... E° = +0.337 V --------------------------------------------------- Ecell = +0.412 V ( 참고 https://ywpop.tistory.com/18119 ) ΔG = –nFEcell ( 참고 https://ywpop.tistory.com/10066 ) = –(2) (96485 C/mol) (0.. 2022. 4. 22.
ΔG 계산. C(s, diamond) → C(s, graphite) ΔG 계산. C(s, diamond) → C(s, graphite) Determine the ΔG and whether the reaction, C(s, diamond) → C(s, graphite), is spontaneous or non-spontaneous. C(s, diamond) + O2(g) → CO2(g) ... ΔG° = –397 kJ C(s, graphite) + O2(g) → CO2(g) ... ΔG° = –394 kJ --------------------------------------------------- ▶ 참고: 헤스의 법칙 [ https://ywpop.tistory.com/3376 ] ※ 헤스의 법칙을 이용한 이런 유형의 문제는 간단한 원리만 이해하면, 끼워 맞추기 ‘놀이’에.. 2022. 4. 9.
standard entropy change CaF2(s) → CaF2(aq) at 298 K standard entropy change CaF2(s) → CaF2(aq) at 298 K Calculate the standard entropy change for the dissolution of CaF2 in water: CaF2(s) → CaF2(aq) at 298 K, if S° of CaF2(s) = 68.87 J/K•mol S° of CaF2(aq) = –80.8 J/K•mol ΔH°_f of CaF2(s) = –1219.6 kJ/mol ΔH°_f of CaF2(aq) = –1208.09 kJ/mol Using the given data, what is the standard free-energy change? --------------------------------------------.. 2022. 2. 6.
293 K에서 0.2699 V, 303 K에서 0.2669 V 293 K에서 0.2699 V, 303 K에서 0.2669 V 아래와 같은 전지의 표준 전지 전위는 293 K에서 0.2699 V이고 303 K에서는 0.2669 V임이 관찰되었다. Pt(s) | H2(g) | HCl(aq) | Hg2Cl2(s) | Hg(l) 298 K에서 다음 반응의 표준 반응 엔트로피의 값은 얼마인가? Hg2Cl2(s) + H2(g) → 2Hg(l) + 2HCl(aq) The standard potential of the cell Pt(s) | H2(g) | HCl(aq) | Hg2Cl2(s) | Hg(l) was found to be +0.2699 V at 293 K and +0.2669 V at 303 K. Evaluate the standard Gibbs energy, enth.. 2022. 1. 3.
methyl isocyanate (CH3NC) isomerizes to acetonitrile (CH3CN) methyl isocyanate (CH3NC) isomerizes to acetonitrile (CH3CN) 기체 상태에서 메틸 이소시아네이트(CH3NC)는 아세토나이트릴(CH3CN)으로 이성화한다. 25℃에서 ΔH° = –89.5 kJ/mol, ΔG° = –73.8 kJ/mol이다. 100℃에서 이 반응의 평형 상수를 찾아라. In the gas phase, methyl isocyanate (CH3NC) isomerizes to acetonitrile (CH3CN), H3C–N≡C(g) ⇌ H3C–C≡N(g) with ΔH° = –89.5 kJ/mol and ΔG° = –73.8 kJ/mol at 25℃. Find the equilibrium constant for this reaction at 100.. 2021. 12. 31.
Boudouard 2CO(g) ⇌ C(s) + CO2(g) 5.07 MPa 1.00 mol% CO Boudouard 2CO(g) ⇌ C(s) + CO2(g) 5.07 MPa 1.00 mol% CO Consider the Boudouard reaction: 2CO(g) ⇌ C(s) + CO2(g) Thermodynamic data on these gases are given in Appendix C. You may assume that ΔH° and ΔS° do not vary with temperature. a) At what temperature will an equilibrium mixture of 101.3 kPa total pressure contain 1.00 mol% CO? b) At what temperature will an equilibrium mixture of 5.07 MPa to.. 2021. 12. 11.
Boudouard 2CO(g) ⇌ C(s) + CO2(g) 101.3 kPa 1.00 mol% CO Boudouard 2CO(g) ⇌ C(s) + CO2(g) 101.3 kPa 1.00 mol% CO Consider the Boudouard reaction: 2CO(g) ⇌ C(s) + CO2(g) Thermodynamic data on these gases are given in Appendix C. You may assume that ΔH° and ΔS° do not vary with temperature. a) At what temperature will an equilibrium mixture of 101.3 kPa total pressure contain 1.00 mol% CO? b) At what temperature will an equilibrium mixture of 5.07 MPa t.. 2021. 12. 11.
25℃ Kw 1.0×10^(-14) ΔG° H2O(l) ⇌ H^+(aq) + OH^-(aq) 25℃ Kw 1.0×10^(-14) ΔG° H2O(l) ⇌ H^+(aq) + OH^-(aq) 25℃ Kw 1.0×10^(-14) ΔG° 2H2O(l) ⇌ H3O^+(aq) + OH^-(aq) Consider the autoionization of water at 25℃. H2O(l) ⇌ H^+(aq) + OH^-(aq) ... Kw = 1.0×10^(-14) Calculate ΔG° for this process at 25℃. --------------------------------------------------- ΔG° = –RT lnK ( 참고 https://ywpop.tistory.com/10336 ) = –(8.314) (273.15 + 25) ln(1.0×10^(-14)) = 79908 J/.. 2021. 12. 10.
ΔG 계산. 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) ΔG 계산. 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) Given that ΔG° = –13.6 kJ/mol, calculate ΔG at 25℃ for the following sets of conditions: P_NH3 = 10 atm P_CO2 = 10 atm [NH2CONH2] = 1.0 M --------------------------------------------------- Q = [NH2CONH2] / ((P_NH3)^2.. 2021. 11. 29.
ΔG 계산. 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) ΔG 계산. 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) ΔG° = –13.6 kJ/mol 반응 조건: 25℃, P_NH3 = P_CO2 = 6.0 atm, [NH2CONH2] = 1.25 M --------------------------------------------------- Q = [NH2CONH2] / ((P_NH3)^2 (P_CO2)) = (1.25) / ((6.0)^2 (6.0)) = 0.005787037 ΔG = ΔG° + RTlnQ ( 참고 https://ywpop.tistory.com/10336 ) = (–13600) + (8.314) (273.15+25) ln(0.005787037) = –26371.2 J/mol = –26.4 kJ/mol 답: –26... 2021. 11. 28.
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