e. 2.89 Calculate the thermodynamic equilibrium constant at 25°C for a reaction for which Δσ.-2560 kJ...
calculate the value for the thermodynamic equilibrium constant for the following reaction. CS2 (g) + 4H2 (g) --> CH4 (g) + 2H2S (g) Values for delta Gf: CS2 (g) --> + 66.85 kJ/mol H2 (g) --> + 0.00 kJ/mol CH4 (g) --> - 50.80 kJ/mol H2S (g) --> - 33.33 kJ/mol R = 8.314 x 10^-3 kJ/molK T = 298 K
Consider the following reaction: A ↔ B Using the thermodynamic data provided below at 25 °C, determine the equilibrium constant for this reaction. R = 8.314 J/mol K . ΔGof(A) = -2.2 kJ/mol ΔGof(B) = -4.8 kJ/mol My key says the correct answer is 2.9, what do you use to get there?
What is ΔrG° for a reaction (in kJ mol-1) which has equilibrium constant K = 1.0 x 1010 at the temperature 16.3 °C? You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
Calculate the equilibrium constant for the following reaction at 25 °C and 150°C. 11. (2) NH CI() NH()HC1(g) NH,C1 (s) -202.87 NH( -16.45 HC1(8) -95.30 AG (kJ-mo1-1) AG [-16.45(-95.0 -202.87] 91.12 kJ At 298 K: K#e*(- Gran/RT) e*(91120/(8.314 x 298) 1.1 At 423 K: K= e"(-aGrin/RT)-e*(91 120/(8.314 x 423) = 5.6 × 10-16 10-12
Calculate the equilibrium constant for the following reaction at 25 °C and 150°C. 11. (2) NH CI() NH()HC1(g) NH,C1 (s) -202.87 NH( -16.45 HC1(8) -95.30 AG...
Given the reference thermodynamic data below taken at 25°C, calculate the value of the equilibrium constant for the reaction shown at 800.0ºC COCl2 (g) ⇄ CO (g) + Cl2 (g) ΔGº = 69.46 kJ ΔHº = 110.38 kJ ΔSº = 137.24 J/K K = Answer at 800.0ºC
What is the equilibrium constant for a reaction at temperature 51.4 °C if the equilibrium constant at 41.6 °C is 13.65? For this reaction, A, H = 10.4 kJ mol-? You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
What is the equilibrium constant for a reaction at temperature 42.5 °C if the equilibrium constant at 19.1 °C is 26.38? For this reaction, AH = 23.8 kJ mol-1 You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
What is the equilibrium constant for a reaction at temperature 87.2 °C if the equilibrium constant at 78.0 °C is 9.82? For this reaction, ΔrH = 14.9 kJ mol-1 . You have 5 attempts at this question. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4".
to t o 10. What is the equilibrium constant of the following reaction at 25°C? 1(s) + 2LiBr(s) 22Lil(s) + Br2(1) AHO=162 kJ mol-1, AS7=61.1 J mol-1 K-1 AGO=143 kJ mol a) 4 x 10-29 b) 1 x 1025 c) 9 x 10-26 d) 3.2 x 102 e) 3.1 x 10-3 11. What is the equilibrium constant of the following reaction at 25°C? Mg(OH)2(aq) + NaOH(aq) + NaOH(aq) + Mg(OH)2(s) a) 1.78 x 1025 -Ox0.1 b) 5.62 x 10-26 c)...
Given the reference thermodynamic data below taken at 25°C, calculate the value of the equilibrium constant for the reaction shown at 800.0°C COCI, (g) 2 CO (g) + Cl2 (g) AG° = 69.46 kJ AH° = 110.38 kJ AS° = 137.24 J/K at 800.0°C