QUESTION 17 1 points [CLO-4] Consider the following equilibrium. 2 SO2(g) + O2 (g) ==== 2...
QUESTION 21 1 point ==== [CLO-4] Consider the following equilibrium. 2 SO2 (g) + O2 (g) 2 S03 (g) The equilibrium cannot be established when [Hint: no need to do any calculations !!!) 1.0 mol SO3 (g) is/are placed in a 1.0-L container 0.75 mol SO2 (g) 0.25 mol SO2 (g) and 0.25 mol O2 (g) 0.50 mol O2 (g) and 0.50 mol SO3(g) 0.25 mol of SO2 (g) and 0.25 mol of SO3(g) Save All Answers Click Save and...
1. Consider the following equilibrium 2SO2 (g O2 (g) 2SOs (g) From which of the following starting conditions would it be impossible for this equilibrium to be achieved? a) 0.25 mol SO2 (g) and 0.25 mol O2 (g) are in a 1.0L container b) 0.75 mol SO2 (g) in al.OL container. c) 0.50 mol O2 (g) and 0.50 mol SOs (g) in al.OL container. d) 1.0 mol SO3 (g) in 1.OL container. The rate law for the decomposition of H2O2...
Consider the following reaction and its equilibrium constant: SO2(g) + NO2(8) - SO3(g) + NO(g) Kc=0.33 A reaction mixture contains 1.0 mol L-1 SO2, 0.50 mol L-1 NO2,0.50 mol L-1 SO3, and 1.0 mol L-1 NO. Which of the following statements is TRUE concerning this system? A) The reaction will shift in the direction of reactants. B) The system is at equilibrium. C) The reaction quotient will decrease. D) The reaction will shift in the direction of products. E) The...
Consider the following equilibrium reaction : Heat + 2 SO2 (g) + O2(g) ↔ 2 SO3(g) Assume the above reaction is allowed to reach equilibrium prior to the following changes. Answer the following questions by writing increase, decrease or remain the same on the line. **please also explain why** If the reaction mixture is heated up , the value of the equilibrium constant will _______________________ If SO2 (g) is added to the reaction vessel the concentration of O2(g) will____________________________. If SO3 (g) is...
3. Consider the following reaction: 2 SO2 (g) + O2 (g) → 2 SO3 (g) AH.x = -197.6 kJ a. If 285.3 g of SO2 is allowed to react with 158.9 g of O2, what is the limiting reactant and theoretical yield of SO3 in liters if the reaction is performed at 315 K and 50.0 mmHg? How much of each reactant remains at the end of the reaction? [10] LR: SO TY: SO2 remaining: O2 remaining: Imol soa 64.000log...
At a certain temperature, 0.780 mol SO2 is placed in a 4.00 L container. 2 SO3(g) = 2 SO2(g) + O2(g) At equilibrium, 0.180 mol O2 is present. Calculate Kc. Kc =
1. Consider the following reaction at equilibrium. 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g) a. What will happen if the pressure increased? b. What will happen if the concentration of FeS2(s) is decreased? 2) The following reaction is exothermic: What direction will the equilibrium shift if the following changes are made? 2 SO2(g) + O2(g) ⇌ 2 SO3(g) a) Raising the temperature b) Adding SO3 c) Removing O2 d) Decreasing the volume
2.5 points Save Ans QUESTION 2 Given the equilibrium, 2SO2(g)+02(g) 2SO 3(g), if this equilibrium, is established by beginning with an equal number of moles of SO2 and O2 in a 1.0 Liter bulb, then the following must be true at equilibrium: O[SO2] [SO3] 2[SO2] = 2[SO3] [SO21 = [02] SO2] < [02]
2) For the equilibrium: 2 SO2(g) + O2(g) < => 2 503(g) Kp = 2.98 at 875oC What is Ke at this temperature? Ko-K[RT]An R = 0.08206 L-atm/mol K (5pts)
For the equilibrium: 2 SO3(g) < = > O2(g) + 2 SO2(g) Kp = 0.269 at 625 oC What is Kc at this temperature? Kp = Kc[RT]Δn R = 0.08206 L-atm/mol K