![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] = 0.5](http://img.homeworklib.com/questions/1a372f50-043b-11ec-b8bd-67a5fb066ab7.png?x-oss-process=image/resize,w_560)
Homework Answers
![リ ke o No net reciction [502] = 0.am [02] = 0.6 M [sog] = 0.6M Q = (0.6) ² (0.2)? (0.6) =(0.36) (0.04) (0.6) equilibrium IQ =](http://img.homeworklib.com/questions/1ade0680-043b-11ec-950a-870fe32951cb.png?x-oss-process=image/resize,w_560)
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At 850 K, the equilibrium constant for the reaction 2 SO, (g) + O2(g) = 250(g)...
At 850 K the equilibrium constant for the following reaction is Ke 15. so,el-ole) 근 sole)...
At 850 K the equilibrium constant for the following reaction is Ke 15. so,el-ole) 근 sole) e mix the following concentrations of the three gases, predict in hich direction the net reaction proceed toward equilibrium. Left No net reaction Right SO]-0.14 M [SO2]-0.70 M [SO2]-0.20 M [02] = 0.20 M [02] = 0.60 M [02] = 0.60 M [SO3] = 0.40 M [SOg] = 0.11 M [SO] = 0.60 M
At 850 K, the equilibrium constant for the reaction 2SO2(g)+O2(g)↽−−⇀2SO3(g)
At 850 K, the equilibrium constant for the reaction 2SO2(g)+O2(g)↽−−⇀2SO3(g) is ?c=15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium.
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
Consider the reaction below at 850 K: 2SO 2 (g)+O 2 (g)⇌2SO 3 ...
Consider the reaction below at 850 K: 2SO 2 (g)+O 2 (g)⇌2SO 3 (g) Kc=15 Now lets think about how the reaction will proceed under the following sets of starting conditions. In each case predict if the reaction will proceed: \textbf{forwards,}forwards, or \textbf{backwards}backwards. [SO2] = 0.15 M, [O_2][O2] = 0.68 M, [SO_3][SO3] = 0.36 M The value of Q is The reaction will proceed [SO_2][SO 2 ] = 0.18 M, [O_2][O 2 ] = 0.10...
The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8...
The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8 x 103 Which direction will the reaction proceed if [502] = 0.015 M. [02] = 0.010 Mand (SO3) = 0.200 M? no shift shifts to make more product shifts to make more reactant
The equilibrium constant for the 2SO2 + O2> 2SO reaction is K = 35.5. Which of...
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 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.
5. At 700 K, the reaction 2solg) + O2(g) 늑 2solg) has the equilibrium constant ....
5. At 700 K, the reaction 2solg) + O2(g) 늑 2solg) has the equilibrium constant . 4.3 106 , and the following concentrations are present: [SO2)-0.10 M: [soi-10. M: [01-0.10 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium? Show how you arrive at your answe below. No work no credit. A. Yes, the mixture is at...
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2]...
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2] = 0.424 [ 2. We place 10.0 moles of N20 into a 2.00 L flask at 300 K. At equilibrium 2.20 moles remain. O2]-0.212 [SO3] = 0.076, find the Kc Given the following reaction, what is the Kc and the concentrations of N2 and O2? 3. Indicate whether the reaction will proceed right or left, and which concentrations will decrease or increase: 2HI(g) 근...
10. A study of the system, 4 NH3(g) + 7 O2(g) 2 N2O4(q) + 6 H2O(g), was carried out. A system was prepared with...
10. A study of the system, 4 NH3(g) + 7 O2(g) 2 N2O4(q) + 6 H2O(g), was carried out. A system was prepared with (NH3) = [02] = 3.60 M as the only components initially. At equilibrium. [N204) is 0.60 M. Calculate the equilibrium concentration of O2. a, 3.00 M b. 2.40 M c. 1.50 M d. 2.10 M e. 3.30 M 11. For the reaction, 2 SO2(g) + O2(g) 2 SO.(a), at 450.0 K the equilibrium constant, Kc, has...
At 850 K the equilibrium constant for the following reaction is Ke 15. so,el-ole) 근 sole) e mix the following concentrations of the three gases, predict in hich direction the net reaction proceed toward equilibrium. Left No net reaction Right SO]-0.14 M [SO2]-0.70 M [SO2]-0.20 M [02] = 0.20 M [02] = 0.60 M [02] = 0.60 M [SO3] = 0.40 M [SOg] = 0.11 M [SO] = 0.60 M
At 850 K, the equilibrium constant for the reaction 2SO2(g)+O2(g)↽−−⇀2SO3(g) is ?c=15. If the given concentrations of the three gases are mixed, predict in which direction the net reaction will proceed toward equilibrium.
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
The reaction and equilibrium constant are provided. 2 SO2(g) + O2(g) 92 SO3(g) K = 5.8 x 103 Which direction will the reaction proceed if [502] = 0.015 M. [02] = 0.010 Mand (SO3) = 0.200 M? no shift shifts to make more product shifts to make more reactant
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.
5. At 700 K, the reaction 2solg) + O2(g) 늑 2solg) has the equilibrium constant . 4.3 106 , and the following concentrations are present: [SO2)-0.10 M: [soi-10. M: [01-0.10 M. Is the mixture at equilibrium? If not at equilibrium, in which direction (as the equation is written), left to right or right to left, will the reaction proceed to reach equilibrium? Show how you arrive at your answe below. No work no credit. A. Yes, the mixture is at...
Lab Exercise #2: Equilibria Problems 1.2S02e) 22S03(e) at 1500 K: If the equilibrium concentrations are [SO2] = 0.424 [ 2. We place 10.0 moles of N20 into a 2.00 L flask at 300 K. At equilibrium 2.20 moles remain. O2]-0.212 [SO3] = 0.076, find the Kc Given the following reaction, what is the Kc and the concentrations of N2 and O2? 3. Indicate whether the reaction will proceed right or left, and which concentrations will decrease or increase: 2HI(g) 근...
10. A study of the system, 4 NH3(g) + 7 O2(g) 2 N2O4(q) + 6 H2O(g), was carried out. A system was prepared with (NH3) = [02] = 3.60 M as the only components initially. At equilibrium. [N204) is 0.60 M. Calculate the equilibrium concentration of O2. a, 3.00 M b. 2.40 M c. 1.50 M d. 2.10 M e. 3.30 M 11. For the reaction, 2 SO2(g) + O2(g) 2 SO.(a), at 450.0 K the equilibrium constant, Kc, has...
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