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Chemistry
- Given the following information below, determine AGxn at equilibrium. 12(g) + Cl2(g) 2 ICI(g) 11 K, = 81.9 (at 298 K) O 1 O +10.9 kJ O -10.9 kJarrow_forwardCalculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.(a) I2(s) + Cl2(g) ⟶ 2ICl(g) ΔG° = −10.88 kJ(b) H2(g) + I2(s) ⟶ 2HI(g) ΔG° = 3.4 kJ(c) CS2(g) + 3Cl2(g) ⟶ CCl4(g) + S2 Cl2(g) ΔG° = −39 kJ(d) 2SO2(g) + O2(g) ⟶ 2SO3(g) ΔG° = −141.82 kJ(e) CS2(g) ⟶ CS2(l) ΔG° = −1.88 kJarrow_forwardCalculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.(a) O2(g)+2F2(g)⟶2OF2(g) ΔG°=−9.2 kJ(b) I2(s)+Br2(l)⟶2IBr(g) ΔG°=7.3 kJ(c) 2LiOH(s)+CO2(g)⟶Li2CO3(s)+H2O(g) ΔG°=−79 kJarrow_forward
- Given the following data, what is the value of ΔGf° (CH3OH(ℓ) at 25°C?CO(g) + 2 H2(g) ⇄ CH3OH(ℓ) K = 1.081 × 10-40ΔGf°(CO) = -137.2 kJ/molarrow_forwardCalculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given. (a) N2O3(g) ⇌ NO(g) + NO2(g) ΔG° = -1.6 kJ (b) SnCl4(l) ⇌ SnCl4(l) ΔG° = 8.0 kJarrow_forward(a) Calculate K at 298 K for the following reaction: 2C(graphite) + O₂(g) = 2CO(g) C(graphite) CO(g) 0₂(g) AG (kJ) f mol 0 -137.2 0arrow_forward
- Calculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.(a) O2(g) + 2F2(g) ⟶ 2OF2(g) ΔG° = −9.2 kJ(b) I2(s) + Br2(l) ⟶ 2IBr(g) ΔG° = 7.3 kJ(c) 2LiOH(s) + CO2(g) ⟶ Li2 CO3(s) + H2 O(g) ΔG° = −79 kJ(d) N2 O3(g) ⟶ NO(g) + NO2(g) ΔG° = −1.6 kJ(e) SnCl4(l) ⟶ SnCl4(l) ΔG° = 8.0 kJarrow_forwardConsider the following system at equilibrium where ΔΗ° = -10.4 kJ, and Kc = 55.6, at 6.98 × 10² K: H₂(g) + I2 (g) → 2HI(g) If the temperature on the equilibrium system is suddenly decreased: The value of K increases Odecreases Oremains the same The value of Qc Ois less thar K is greater than Kc [References] Ois equal to Kc The reaction must Orun in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium Oremain in the current position, since it is already at equilibrium The concentration of I2 will Cincrease Odecrease Oremain the samearrow_forward(28) The standard Gibbs free energy associated with the following reaction is -91.2 kJ: HCI (g) + NH3 (g) → NH,CI (s) What will be the value of AG,nn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atm and the partial pressure of NH3 (g) is 0.284 atm? (A) (B) -95.1 kl -90.7 kl (C) (D) (E) 3.93 kJ noltemol or ni lu bluos noinsou -79.5 kJ -87.3 kJarrow_forward
- Calculate ΔG° for each of the following reactions from the equilibrium constant at the temperature given. (a) CO2(g) + H2(g) ⇌ CO(g) + H2O(g) t = 980°C Kp = 1.67 (b) CaCO3(s) ⇌ CaO(s) + CO2(g) t = 900°C Kp = 1.04arrow_forwardConsider the same reaction as in the previous question: HNO₂(aq) = H(aq) + NO₂ (aq), AG 19.1 kJ/mol. What is the value of the equilibrium constant for this reaction at 298 K? = (A) 284 (B) 19.1 (C) 0.152 (D) 7.25×10-2 (E) 4.49×10-4arrow_forwardCalculate the equilibrium constant at 25 C for each of the following reactions from the value G given. (a) I2(s)+Cl2(l)2ICl(g)G=10.88kJ (b) H2(g)+I2(s)2HI(g)G=3.4kJ (c) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)G=39kJ (d) 2SO2(g)+O2(g)2SO3(g)G=141.82kJ (e) CS2(g)CS2(l)G=1.88kJarrow_forward
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