13 Question The equilibrium constant for the reaction below decreases from 13540.0 at 570.0°C to 17.0 at 860.0°C. 4NO(g) +30₂(g) 2N₂O(g) 7th attempt T From these data, calculate the value of AH° for the reaction. kJ
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- Given the following two measurements of the equilibrium constant for a reaction, calculate ΔH° for the reaction. (kJ/mol) (no scientific notation) T, °C K 30.0 5.2 x 103 50.0 15.4 x 104At a certain temperature, Kp for the reaction, F2(g) ⇌ 2 F(g) is 0.000849. Calculate the value of Kp for the reaction, 2 F(g) ⇌ F2(g). *The answer is 1.178E3, but would like an explanation*When the following reaction (NH4)2CO3 (s) ↔ 2 NH3 (g) + CO2 (g) + H2O (g) takes place at 65 ºC at 1 atm pressure is obtained.a) Calculate Kp at that temperature and at 25 ºC. (ΔH = 224.82 kJ/mol)b) Calculate XNH3 when the reaction takes place at 25 ºC y 100 mmHg. Result: a) 0.0156, 3.373 10-7 b) 0.259
- Calculate the values of Kp and K at 525°C with the equilibrium pressure of CO2 at 0.220atm for the following reaction.CaCO3 (s) - CaO (s) + CO2 (g)Determine the equilibrium constant for the following reaction at 25 deg. C: 2I- (aq) + Br2(l) --> I2(s) + 2Br-(aq). (Example of answer: 6.5 x 10e-12, where 12 is exponent)For the reaction 6 N2O (g) = 6 N2 (g) + 3 O2 (g), Kp = 0.324 at a temperature of 298 K. What is Kp for the following reaction (with 3 significant figures)? (Choose one option only.) 2 N2 (g) + O2 (g) = 2 N2O (g) Options: a. 0.0340 b. 0.108 c. 9.76 d. 0.687 e. 1.46
- If the value of the equilibrium constant, Kc, for the following reaction is 5.00 × 105 at 298 K, what is the value of Kp at 298 K? 2CO(g)+O2 (g)2CO2 (g)An equilibrium reaction, A2(g) + 3B2(g) 2C(g), has a Kp at 225°C of 4.5 × 10–3 /atm2. What is K for this reaction at that temperature? Group of answer choices 2.7 × 10–6 1.3 × 10–5 7.5 1.1 × 10–4 2.716. What is the numerical value of K, the equilibrium constant, for a reaction with a Δ Go of -56 kJ at 273K? Group of answer choices A 5.2 x 10+10 B 1.9 x 10-11 C 11.8 D 1.02
- The value of the equilibrium constant Kp for the reaction below is 0.873 at 900°C.H2(g)+CO2(g) ----> H2O(g)+CO(g) <---- Calculate the value of ΔG° for the reaction.The equilibrium constant, Kc, for the following reaction is 5.10×10-6 at 548 K. Calculate Kp for this reaction at this temperature. NH4Cl(s)----> NH3(g) + HCl(g)Question 4 Determine the equilibrium constant for the following reaction at 382 °C. HCN (g) + 2 H2 (g) ⇌ CH3NH2 (g) ΔH° = –158 kJ; ΔS° = –219.9 J/K ANSWER:13.0 Just need Part 2 Is there a temperature at which equilibrium for the reaction in Question 4 will "jump the arrows?" Why or why not? If you determined that temperature will shift the position of the equilibrium for this reaction, at what temperature will that occur?