Bromine monochloride is synthesized using the reaction
A flask initially contains of and of Calculate the mass of , in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior.
mass of : ______g
What is the percent yield of
Bromine monochloride is synthesized using the reaction Br2(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 203.0 L flask initially contains 1.070 kg of Br, and 1.115 kg of Cl. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: g What is the percent yield of BrCl? percent yield: %
uestion 16 of 16 > Bromine monochloride is synthesized using the reaction Br (8) + Cl2(g) = 2 BrCl(9) Ko = 1.1 x 10-4 at 150 K A 203.0 L flask initially contains 1.005 kg of Br, and 1.155 kg of Cl. Calculate the mass of BrCI, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of Brci: What is the percent yield of BrCl? percent yield: terms of use contact us help...
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 190.0 L flask initially contains 1.078 kg of Br, and 1.068 kg of Cl.. Calculate the mass of BrCl,, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCI: g What is the percent yield of BrCl? percent yield:
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(g) = 2 BrCI(g) K= 1.1 x 10- at 150 K A 194.0 L flask initially contains 0.905 kg of Br, and 1.101 kg of Cl. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCI: 8 What is the percent yield of BrCl? percent yield: %
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(8) 2 BrCI(g) K, = 1.1 x 10-4 at 150 K A 193.0 L flask initially contains 0.985 kg of Br, and 1.027 kg of Cl. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: 16.0424 Incorrect What is the percent yield of BrCl? % percent yield: 86.7 Incorrect
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) K = 1.1 x 10-4 at 150 K A 197.0 L flask initially contains 1.013 kg of Br, and 1.025 kg of Cl. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCI: g What is the percent yield of BrCl? percent yield: % about us Careers privacy policy terms of use contact us...
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...
Calculate DH for the reaction BrCl(g) -----> Br(g) + Cl(g) Given Br2(l) -----> Br2(g) DH = 30.91 kJ Br2(g) -----> 2Br(g) DH = 192.9 kJ Cl2(g) ------> 2Cl(g) DH = 243.4 kJ Br2(l) + Cl2(g) ----> 2BrCl(g) DH = 29.2 kJ
Consider the following reaction: Br2(g)+Cl2(g)⇌2BrCl(g) Kp=1.11×10−4 at 150 K. A reaction mixture initially contains a Br2 partial pressure of 760 torr and a Cl2 partial pressure of 740 torr at 150 K. Part A Calculate the equilibrium partial pressure of BrCl.
24-18. Consider the reaction described by Cl2 + Br2 -> 2BrCl at 500 K and a total pressure of one bar. Suppose that we start with one mole each Cl2 and Br2 and no BrCl. Show that 24-18. Consider the reaction described by Cl2 (g) + Br2 (g) 2 BrCl(g) at 500 K and a total pressure of one bar. Suppose that we start with one mole each of Cl2(g) and Br (g) and no BrCI(g). Show that where ξ...