Consider the following reaction, 2AB (g) ⇌ A2 (g) + B2 (g) K = 1.50x10−2 At some point in the reaction, Q = 5.30. Which of the following statements is correct concerning the equilibrium? 0.60 mol of Br2 and 0.60 mol of Cl2 are placed in a 1.00 L flask and allowed to reach equilibrium. After reaching equilibrium, the flask is found to contain 0.28 mol of BrCl. What is the value of Kc for this reaction? Br2 (g) + Cl2 (g)...
13/13 pts Question 14 The reaction of bromine gas with chlorine gas, Br,(g)+C12(g) 2 BrClg), has a Kp value of 7.20. If the initial partial pressures of Br2, Cl2, and BrCl in a closed container are all 0.500 atm, what is the equilibrium partial pressure of BrCl(g)? rect! 0.859 atm
Suppose a 250. mL. flask is filled with 1.8 mol of Cl2 and 0.60 mol of HCl. The following reaction becomes possible: H(+Cl()2HCI) The equilibrium constant K for this reaction is 8.25 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 0.90 mol of OC1,, 0.20 mol of BroCl and 1.4 mol of BrCl. The following reaction becomes possible: Br2(g) +OC12(g) =BroCl(g) +BrCl(g) The equilibrium constant K for this reaction is 0.798 at the temperature of the flask. Calculate the equilibrium molarity of Br2. Round your answer to two decimal places. IM xs ?
Suppose a 500. ml flask is filled with 1.3 mol of Br2, 2.0 mol of OC1, and 1.2 mol of BrCl. The following reaction becomes possible: Br2(g) + OC12(g) = BroCl (g) + BrCl (g) The equilibrium constant K for this reaction is 0.766 at the temperature of the flask. Calculate the equilibrium molarity of OC12. Round your answer to two decimal places. xs ?
Suppose a 500 ml flask is filled with 0.10 mol of Bry, 1.6 mol of OCI, and 0.60 mol of BrCl. The following reaction becomes possible: Bry()+OCI (8) -BrOCI () + BrCl() The equilibrium constant K for this reaction is 0.770 at the temperature of the flask Calculate the equilibrium molarity of OCI. Round your answer to two decimal places x x 5 ?
Suppose a 250. mL flask is filled with 1.0 mol of Br,, 1.5 mol of OCI, and 1.8 mol of BrOCI, The following reaction becomes possible: Br (8)+OCI,(8)BroCI (e) + BrCl(e) The equilibrium constant K for this reaction is 0.913 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places.
Suppose a 250. ml flask is filled with 1.8 mol of OC1, 0.70 mol of BroCl and 0.50 mol of BrCl. The following reaction becomes possible: Br2(g) + OC12(g) – Brocl(g) +BrCl(g) The equilibrium constant K for this reaction is 1.48 at the temperature of the flask. Calculate the equilibrium molarity of BroCl. Round your answer to two decimal places. x 5 ?
At 400 K, the equilibrium constant for the reaction Br 2 (g) + Cl 2 (g) 2BrCl (g) is K p = 7.0. A closed vessel at 400 K is charged with 1.00 atm of Br 2 (g), 1.00 atm of Cl 2 (g), and 2.00 atm of BrCl (g). Use Q to determine which of the statements below is true. The equilibrium partial pressures of Br2, Cl2, and BrCl will be the same as the initial values. The reaction will...
Bromine monochloride is synthesized using the reactionBr2(g)+Cl2(g)↽−−⇀2BrCl(g)?p=1.1×10−4 at 150 KBr2(g)+Cl2(g)↽−−⇀2BrCl(g)Kp=1.1×10−4 at 150 KA 203.0 L203.0 L flask initially contains 0.986 kg of Br2Br2and 1.088 kg of Cl2.Cl2. Calculate the mass of BrClBrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior.mass of BrClBrCl: ______gWhat is the percent yield of BrCl?percent yield: _________%