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Using data from the table below, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K. AG (kJ/mol) Substance NaHCO3 (s) -851.8 NaOH(s) -379.5 CaCO3(s) -1128.76 CaO(s) -604.0 K₂CO3(s) -1064.58 K₂O(s) -322.1 CO₂ (g) HBr(g) HCl(g) Br₂ (g) SO₂(g) -300.4 SO3(g) <-370.4 CO(g) -394.4 -53.34 -95.27 3.14 -137.2 CH3OH(g) -161.9 NO(g) NO₂ (g) 86.71 51.84 ▶ ▼ Part E Part F 2HBr(g) + Cl₂ (g) = 2HCl(g) + Br2 (g) Calculate the value of the equilibrium constant. Express the equilibrium constant to three significant figures. K= Submit ▶ Part G Part H AG° = - ΑΣΦ Submit Request Answer 2NO(g) + O2(g) = 2NO₂(g) What is the free-energy change for these reactions at 298 K? Express the free energy in kilojoules to one decimal place. 195| ΑΣΦ ? Request Answer ? kJ

Using data from the table below, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K. AG (kJ/mol) Substance NaHCO3 (s) -851.8 NaOH(s) -379.5 CaCO3(s) -1128.76 CaO(s) -604.0 K₂CO3(s) -1064.58 K₂O(s) -322.1 CO₂ (g) HBr(g) HCl(g) Br₂ (g) SO₂(g) -300.4 SO3(g) <-370.4 CO(g) -394.4 -53.34 -95.27 3.14 -137.2 CH3OH(g) -161.9 NO(g) NO₂ (g) 86.71 51.84 ▶ ▼ Part E Part F 2HBr(g) + Cl₂ (g) = 2HCl(g) + Br2 (g) Calculate the value of the equilibrium constant. Express the equilibrium constant to three significant figures. K= Submit ▶ Part G Part H AG° = - ΑΣΦ Submit Request Answer 2NO(g) + O2(g) = 2NO₂(g) What is the free-energy change for these reactions at 298 K? Express the free energy in kilojoules to one decimal place. 195| ΑΣΦ ? Request Answer ? kJ

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
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Using data from the table below, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K. AG (kJ/mol) Substance NaHCO3(s) -851.8 NaOH(s) -379.5 CaCO3(s) -1128.76 | CaO(s) -604.0 K₂CO3(s) -1064.58 K₂O(s) -322.1 CO₂ (g) HBr(g) HCl(g) Br₂ (g) SO₂(g) SO3(g) GO(g) -394.4 -53.34 -95.27 3.14 -300.4 -370.4 -137.2 CH3OH(g) -161.9 NO(g) NO₂ (g) 86.71 51.84 ▶ ▼ Part E Part F 2HBr(g) + Cl₂ (g) = 2HCl(g) + Br2 (g) Calculate the value of the equilibrium constant. Express the equilibrium constant to three significant figures. K= Submit ▶ Part G Part H AG° = - ΑΣΦ Submit Request Answer 2NO(g) + O2(g) = 2NO₂(g) What is the free-energy change for these reactions at 298 K? Express the free energy in kilojoules to one decimal place. 5. ΑΣΦ ? Request Answer ? kJ
Transcribed Image Text:Using data from the table below, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K. AG (kJ/mol) Substance NaHCO3(s) -851.8 NaOH(s) -379.5 CaCO3(s) -1128.76 | CaO(s) -604.0 K₂CO3(s) -1064.58 K₂O(s) -322.1 CO₂ (g) HBr(g) HCl(g) Br₂ (g) SO₂(g) SO3(g) GO(g) -394.4 -53.34 -95.27 3.14 -300.4 -370.4 -137.2 CH3OH(g) -161.9 NO(g) NO₂ (g) 86.71 51.84 ▶ ▼ Part E Part F 2HBr(g) + Cl₂ (g) = 2HCl(g) + Br2 (g) Calculate the value of the equilibrium constant. Express the equilibrium constant to three significant figures. K= Submit ▶ Part G Part H AG° = - ΑΣΦ Submit Request Answer 2NO(g) + O2(g) = 2NO₂(g) What is the free-energy change for these reactions at 298 K? Express the free energy in kilojoules to one decimal place. 5. ΑΣΦ ? Request Answer ? kJ
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