Exercise 4-The Equilibrium Constant, Enthalpy and Free Energy of Formation The following reaction was carried out i...
A) The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl2(g) <->CH4(g) + CCl4(g) If an equilibrium mixture of the three gases in a 19.9 L container at 350K contains 0.416 mol of CH2Cl2(g) and 0.202 mol of CH4, the equilibrium concentration of CCl4 is B) 2SO3(g) <->2SO2(g) + O2(g) If 0.184 moles of SO3(g), 0.477 moles of SO2, and 0.234 moles of O2 are at equilibrium in a 15.0 L container at 1.23×103 K, the value...
Calculate the equilibrium constant for the reaction below if a 5.50 L tank contains 0.526 mol O2, 0.1032 mol SO3 and 0.01658 mol SO2. 2SO3 (g) ↔ 2SO2 (g) + O2 (g)
The equilibrium constant for the 2SO2 + O2> 2SO reaction is K = 35.5. Which of the following statements are correct when 0.10 mol SO2, 0.20 mol O2 and 0.052 mol SO3 are put in a 2.0 liter container? Reaction I is in equilibrium. II. The reaction is forward. III. SO3 (g) concentration increases. IV. O2 concentration decreases. answer:2,3,4
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to form SO3 is 0.365 at 1.15×103 K: SO2(g) + O2(g) = 2SO3(g) A sample of SO3 is introduced into an evacuated container at 298 K and allowed to dissociate until its partial pressure reaches an equilibrium value of 0.867 atm. Calculate the equilibrium partial pressures of SO2 and O2 in the container. PSO2 = PO2 =
If the equilibrium constant for reaction X is K. What is the equilibrium constant for reaction Y is? Reaction X: SO2 (g) + (1/2) O2 (g) ⇌ SO3 (g) Reaction Y: 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) a. 2K b. K2 c. 1/K2 d. 0.5 x K e. -K2
At a given temperature, the equilibrium constant Kc for the reaction 2SO2(g)+O2(g)<==>2SO3(g) is 2.99x10^-3. What is the value of the equilibrium constant for each of the following reactions at that temperature? a. SO2(g)+ 1/2 O2(g)<==> SO3(g) b. 2SO3(g)<==>2SO2(g)+O2(g) c. SO3(g)<==> SO2(g)+ 1/2 O2(g)
Consider the reaction listed below along with the accompanying thermodynamic data, carried out at 25 °C and 1 atm: 2SO2(g) + O2(g) ↔ 2SO3(g) Substance ∆Hf° (kJ/mol) S° (J/K • mol) SO2(g) -297 248 O2(g) 0 205 SO3(g) -396 257 A.Calculate ∆H°. B. Calculate ∆S°. C. Calculate ∆G°. Is this reaction spontaneous? Briefly explain. D. At what temperature will this reaction first become spontaneous? E. Calculate the equilibrium constant for this reaction.
The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 7 × 103 at a certain temperature. If at equilibrium, [SO2] = 0.0451 M and [O2] = 0.078 M, what is the equilibrium [SO3]?
Enter your answer in the provided box. The formation of SO3 from SO2 and O2 is an intermediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. The equilibrium constant KP for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 0.13 at 803°C. In one experiment, 2.00 mol SO2 and 2.00 mol O2 were initially present in a flask. What must be the total pressure at equilibrium in order to have an...
A 2.0 L flask is filled with 0.30 mol SO3 , 0.40 mol of SO2 and 0.50 mol of O2 and allowed to reach equilibrium. Assume the temperature of the mixture is chosen so that Kc = 0.34. Predict the effect on the concentration of SO3 as the equilibrium is achieved by using Q, the reaction quotient. 2SO3(g) —> 2SO2(g) + O2(g)