Homework Answers
Here, Kc= [SO3]^2/[SO2]^2[O2]= 1.77*10^4
Since the new Kc is larger, means that the reactant is less than the product. So, it will shift towards left to make more reactant.
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The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8...
5 pts Question 3 The reaction and equilibrium constant are provided. 2 SO2 (9) + O2...
5 pts Question 3 The reaction and equilibrium constant are provided. 2 SO2 (9) + O2 (g) 92 SO3 (g) Kc = 5.8 x 103 Which direction will the reaction proceed if [SO2] = 0.15 M, [O2] = 0.10 M and (SO3) = 0.50 M? shifts to make more reactant shifts to make more product no shift
At 850 K, the equilibrium constant for the reaction 2 SO, (g) + O2(g) = 250(g)...
At 850 K, the equilibrium constant for the reaction 2 SO, (g) + O2(g) = 250(g) is Kc = 15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium. Left No net reaction Right Answer Bank [S02] = 0.20 M [02] = 0.60 M [SO3) = 0.60 M [SO2] = 0.21 M [02] = 0.10 M [SO3] = 0.60 M [SO2] = 0.80 M [02] = 0.50 M...
27. Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = SO3(g) + NO(g)...
27. Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = SO3(g) + NO(g) Kc = 0.33 A reaction mixture contains 0.41 M SO2, 0.13 M NO2.0.11 M SO3 and 0.13 M NO. Which of the following statements is TRUE concerning this system? A) The reaction will shift in the direction of reactants. B) The equilibrium constant will decrease. C) The reaction will shift in the direction of products. D) The reaction quotient will decrease. E) The system...
5. For the reaction... SO2 + O2 <=> SO3 If the equilibrium position shifts to the...
5. For the reaction... SO2 + O2 <=> SO3 If the equilibrium position shifts to the right, the concentration of O2 will (2 points) o remain constant increase Decrease
The equilibrium constant in terms of pressures, Kp, for the reaction of SO2 and O2 to...
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 =
1.For the reaction at equilibrium 2 SO3↔ 2 SO2 + O2 (∆Horxn= 198 kJ/mol), if we...
1.For the reaction at equilibrium 2 SO3↔ 2 SO2 + O2 (∆Horxn= 198 kJ/mol), if we increase the reaction temperature, the equilibrium will (1 point ) * No shift None of the above Question lacks sufficient information Shift to the right 2. For the equilibrium reaction 2 SO2(g) + O2(g) ↔ 2 SO3(g), ∆Horxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase? (1 point ) * Add a catalyst Decrease the temperature None...
Consider the following reaction and its equilibrium constant: SO2(g) + NO2(8) - SO3(g) + NO(g) Kc=0.33...
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...
The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2502(g) + O2(g)...
The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2502(g) + O2(g) = 2503(g) If initial concentrations are [SO2] = 10.8 M, [O2] = 0.45 M, and (SO3) = 16.2 M, the system is not at equilibrium and will remain in an unequilibrated state. not at equilibrium and will shift to the left to achieve an equilibrium state. O at equilibrium. not at equilibrium and will shift to the right to achieve an equilibrium state.
10) The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 10) 2 SO2(8) + O2(8) - 2 SO3(3). If initi...
10) The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 10) 2 SO2(8) + O2(8) - 2 SO3(3). If initial concentrations are [SO2) = 6.00 M, [02] -0.45 M, and (SO3) = 9.00 M, the system is A) not at equilibrium and will shift to the right to achieve an equilibrium state. B) not at equilibrium and will shift to the left to achieve an equilibrium state. C) at equilibrium D) not at equilibrium and will...
The equilibrium constant for the following reaction is 1.71×10-2 at 847 °C. 2 SO3(g)2 SO2(g) +...
The equilibrium constant for the following reaction is 1.71×10-2 at 847 °C. 2 SO3(g)2 SO2(g) + O2(g) K = 1.71×10-2 at 847 °C Calculate the equilibrium constant for the following reactions at 847 °C. (a) 2 SO2(g) + O2(g)2 SO3(g) K = (b) SO3(g) SO2(g) + 1/2 O2(g) K = Show Approach
5 pts Question 3 The reaction and equilibrium constant are provided. 2 SO2 (9) + O2 (g) 92 SO3 (g) Kc = 5.8 x 103 Which direction will the reaction proceed if [SO2] = 0.15 M, [O2] = 0.10 M and (SO3) = 0.50 M? shifts to make more reactant shifts to make more product no shift
At 850 K, the equilibrium constant for the reaction 2 SO, (g) + O2(g) = 250(g) is Kc = 15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium. Left No net reaction Right Answer Bank [S02] = 0.20 M [02] = 0.60 M [SO3) = 0.60 M [SO2] = 0.21 M [02] = 0.10 M [SO3] = 0.60 M [SO2] = 0.80 M [02] = 0.50 M...
27. Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) = SO3(g) + NO(g) Kc = 0.33 A reaction mixture contains 0.41 M SO2, 0.13 M NO2.0.11 M SO3 and 0.13 M NO. Which of the following statements is TRUE concerning this system? A) The reaction will shift in the direction of reactants. B) The equilibrium constant will decrease. C) The reaction will shift in the direction of products. D) The reaction quotient will decrease. E) The system...
5. For the reaction... SO2 + O2 <=> SO3 If the equilibrium position shifts to the right, the concentration of O2 will (2 points) o remain constant increase Decrease
The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2502(g) + O2(g) = 2503(g) If initial concentrations are [SO2] = 10.8 M, [O2] = 0.45 M, and (SO3) = 16.2 M, the system is not at equilibrium and will remain in an unequilibrated state. not at equilibrium and will shift to the left to achieve an equilibrium state. O at equilibrium. not at equilibrium and will shift to the right to achieve an equilibrium state.
10) The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 10) 2 SO2(8) + O2(8) - 2 SO3(3). If initial concentrations are [SO2) = 6.00 M, [02] -0.45 M, and (SO3) = 9.00 M, the system is A) not at equilibrium and will shift to the right to achieve an equilibrium state. B) not at equilibrium and will shift to the left to achieve an equilibrium state. C) at equilibrium D) not at equilibrium and will...
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