![QUESTION 2 CO(g) + Cl2(g) = COCI_(a) Kc - 1.2 x 10 at 400 °C Consider the above reaction. If the (CO) = [C12] = [COC12] = 5 x](http://img.homeworklib.com/questions/d575ccf0-981b-11eb-b353-7bf23a91d5e5.png?x-oss-process=image/resize,w_560)
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![For the reaction Cig (9) coci (1) to (9) teociz) [co] [12] 2x104 5 x10-5 (5x10-52 Rec 2 xlou ® OY K tence reaction will 3 Sin](http://img.homeworklib.com/questions/d7d4d2f0-981b-11eb-bca1-b5e1e08c4e28.png?x-oss-process=image/resize,w_560)
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QUESTION 2 CO(g) + Cl2(g) = COCI_(a) Kc - 1.2 x 10 at 400 °C Consider...
Consider this reaction: CO(g) + Cl2(g) - COC12(g) where Kp at 1000 K is 3.9 x...
Consider this reaction: CO(g) + Cl2(g) - COC12(g) where Kp at 1000 K is 3.9 x 10-2 If the reaction mixture initially contains 0.2 atm CO, 0.2 atm Cl2. and 0.1 atm CoCl2, which direction will the reaction proceed? to the left to the right
Tutored Practice Problem 16.4.1 COUNTS TOWARDS GRADE Predict and calculate the effect of concentration changes on...
Tutored Practice Problem 16.4.1 COUNTS TOWARDS GRADE Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some COCl2 is allowed to dissociate into CO and Cl2 at 873 K. At equilibrium, [COCI2] =0.237 M, and [CO] - [C12] = 0.128 M. Additional CO is added so that (CO)new = 0.193 M and the system is allowed to once again reach equilibrium. COC12(8) CO(g) + Cl2(g) K-6.98*10-2 at 873K (a) In which direction will the reaction...
Consider the following reaction where Kc = 1.29x10^-2 at 600 K: CO(g) + Cl2(g) --> COCl2(g)...
Consider the following reaction where Kc = 1.29x10^-2 at 600 K: CO(g) + Cl2(g) --> COCl2(g) A reaction mixture was found to contain 5.48x10^-2 moles of CO(g), 3.74×10^-2 moles of Cl2(g) and 0.114 moles of COCl2(g), in a 1.00 Liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium COCl2(g) must be produced. 2. In order to reach equilibrium Kc must decrease. 3. In order to reach equilibrium CO must be...
Consider the equilibrium between COCl2, CO and Cl2. COCl2(g) CO(g) + Cl2(g) K = 0.112 at...
Consider the equilibrium between COCl2, CO and Cl2. COCl2(g) CO(g) + Cl2(g) K = 0.112 at 904 K The reaction is allowed to reach equilibrium in a 7.00-L flask. At equilibrium, [COCl2] = 0.258 M, [CO] = 0.170 M and [Cl2] = 0.170 M. (a) The equilibrium mixture is transferred to a 14.0-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a...
Consider the following reaction: COCl2(g) = CO(g) + Cl2(8) A reaction mixture initially contains 1.6 M...
Consider the following reaction: COCl2(g) = CO(g) + Cl2(8) A reaction mixture initially contains 1.6 M COC12. Determine the equilibrium concentrations of COCI, CO, and Cl2 if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. Use x is small approximation. Show Q Validity check [Cl2] = [CO]= [COCI2] = Calculate the reaction quotient, Q A % Validity Check A Calculate the A/ equilibrium...
Consider the following reaction where Ke = 1.29x10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) A...
Consider the following reaction where Ke = 1.29x10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) A reaction mixture was found to contain 9.63x10-2 moles of COC1(2), 4.64x10-2 moles of CO(g), and 3.72x10-2 moles of Cl(), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse...
Consider the equilibrium between PCls, PClj and Cl2. PCIs(g)-PC13(g) + Cl2(g) K 0.251 at 571 K...
Consider the equilibrium between PCls, PClj and Cl2. PCIs(g)-PC13(g) + Cl2(g) K 0.251 at 571 K The reaction is allowed to reach equilibrium in a 15.2-L flask. At equilibrium, [PCIs]-9.75x102 M, [PCl,]-o.156 M and [C12] = 0.156 M. (a) The equilibrium mixture is transferred to a 7.60-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 7.60-L flask. [PCI5] [C12] =
2. Consider the following system at equilibrium where H° = 108 kJ/mol, and Kc = 1.29×10-2,...
2. Consider the following system at equilibrium where H° = 108 kJ/mol, and Kc = 1.29×10-2, at 600 K. COCl2(g) CO (g) + Cl2(g) When 0.19 moles of COCl2(g) are removed from the equilibrium system at constant temperature: The value of Kc _________increases.decreases.remains the same. The value of Qc _________is greater than is equal to is less than Kc. The reaction must run in the forward direction to reestablish equilibrium. run in the reverse direction to reestablish equilibrium. remain the...
please show all steps. The decomposition reaction of COC12 is, COCldg,-CO(g) + Cl2(g) Kc = 2.2...
please show all steps.
The decomposition reaction of COC12 is, COCldg,-CO(g) + Cl2(g) Kc = 2.2 × 10-10. The initial concentration of CoCl is 0.3166 M 3. the (a) At equilibrium, the concentrations of the products are concentration of reactant. (A) greater than (B) less than (D) unknown because more information is needed to determine. (C) equal to (b) Fill the ICE table below COC: Ico Initial concentration (M) Changes (M) Equilibrium concentration (M) -x (c) Calculate the equilibrium concentration...
At 100 °C the equilibrium constant for the reaction COCI2 (g) CO (g) +Cl2 (g) has...
At 100 °C the equilibrium constant for the reaction COCI2 (g) CO (g) +Cl2 (g) has the value Ke following mixtures of COCI2, CO, and Cl2 at 100 °C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. 2.19 x 1010. Are the Part A 3.3 x 10-6 M. [Cl2] = 6.62 x 10- M [COCI2] = 2.00 x 10-3 M. [CO] The reaction is at equilibrium. The reaction will proceed right to attain...
Consider this reaction: CO(g) + Cl2(g) - COC12(g) where Kp at 1000 K is 3.9 x 10-2 If the reaction mixture initially contains 0.2 atm CO, 0.2 atm Cl2. and 0.1 atm CoCl2, which direction will the reaction proceed? to the left to the right
Tutored Practice Problem 16.4.1 COUNTS TOWARDS GRADE Predict and calculate the effect of concentration changes on an equilibrium system. Close Problem Some COCl2 is allowed to dissociate into CO and Cl2 at 873 K. At equilibrium, [COCI2] =0.237 M, and [CO] - [C12] = 0.128 M. Additional CO is added so that (CO)new = 0.193 M and the system is allowed to once again reach equilibrium. COC12(8) CO(g) + Cl2(g) K-6.98*10-2 at 873K (a) In which direction will the reaction...
Consider the following reaction: COCl2(g) = CO(g) + Cl2(8) A reaction mixture initially contains 1.6 M COC12. Determine the equilibrium concentrations of COCI, CO, and Cl2 if Kc for the reaction at this temperature is 8.33 x 10-4. Calculate this based on the assumption that the answer is negligible compared to 1.6. Use x is small approximation. Show Q Validity check [Cl2] = [CO]= [COCI2] = Calculate the reaction quotient, Q A % Validity Check A Calculate the A/ equilibrium...
Consider the following reaction where Ke = 1.29x10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) A reaction mixture was found to contain 9.63x10-2 moles of COC1(2), 4.64x10-2 moles of CO(g), and 3.72x10-2 moles of Cl(), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qc equals The reaction A. must run in the forward direction to reach equilibrium. B. must run in the reverse...
Consider the equilibrium between PCls, PClj and Cl2. PCIs(g)-PC13(g) + Cl2(g) K 0.251 at 571 K The reaction is allowed to reach equilibrium in a 15.2-L flask. At equilibrium, [PCIs]-9.75x102 M, [PCl,]-o.156 M and [C12] = 0.156 M. (a) The equilibrium mixture is transferred to a 7.60-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 7.60-L flask. [PCI5] [C12] =
please show all steps.
The decomposition reaction of COC12 is, COCldg,-CO(g) + Cl2(g) Kc = 2.2 × 10-10. The initial concentration of CoCl is 0.3166 M 3. the (a) At equilibrium, the concentrations of the products are concentration of reactant. (A) greater than (B) less than (D) unknown because more information is needed to determine. (C) equal to (b) Fill the ICE table below COC: Ico Initial concentration (M) Changes (M) Equilibrium concentration (M) -x (c) Calculate the equilibrium concentration...
At 100 °C the equilibrium constant for the reaction COCI2 (g) CO (g) +Cl2 (g) has the value Ke following mixtures of COCI2, CO, and Cl2 at 100 °C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. 2.19 x 1010. Are the Part A 3.3 x 10-6 M. [Cl2] = 6.62 x 10- M [COCI2] = 2.00 x 10-3 M. [CO] The reaction is at equilibrium. The reaction will proceed right to attain...
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