The equilibrium constant Kc for the reaction below is 0.00491 at a certain temperature. If the initial concentrations are [Br2l-0.0860 M and [Br concentrations of these species at equilibrium. 0.0362...
The equilibrium constant Kc for the reaction below is 0.00384 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0257 M and [Br] = 0.0888 M, calculate the concentrations of these species at equilibrium.
The equilibrium constant for the reaction below is Kc=115. if the initial concentrations of F2, H2 and HF are all 2.0 M, what are the equilibrium concentrations of H2 and HF? F2(g) + H2(g) <--> 2HF(g)
Be sure to answer all parts. At 1280°C the equilibrium constant Kc for the reaction Br2(g) ⇌ 2Br(g) is 1.1 × 10−3. If the initial concentrations are [Br2] = 0.0390 M and [Br] = 0.0370 M, calculate the concentrations of these two species at equilibrium. [Br2]eq [Br]eq
At 1280°C the equilibrium constant Kc for the reaction Br2(g) ⇌ 2Br(g) is 1.1 × 10−3. If the initial concentrations are [Br2] = 0.0480 M and [Br] = 0.0470 M, calculate the concentrations of these two species at equilibrium. [Br2]eq = ___M [Br]eq = ____M
Consider the reaction below. The initial concentration of KBr is 0.0183 M, and the initial concentrations of K+ and Br− are each 0 M. If the equilibrium constant is Kc=7.76 under certain conditions, what is the equilibrium concentration of KBr? KBr(aq)⇌K+(aq)+Br−(aq) Remember to use correct significant figures in your answer (round your answer to the nearest hundredth).
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3 A(g) + 2 B(g) = 4C(g) Kc = 2.93 x 1015 If, at this temperature, 1.40 mol of A and 3.90 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = 0 B) = 1.8667 [C] = | 2.967
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3 A(g) + 2B(g) = 4C(g) K. = 2.93 x 1017 If, at this temperature, 1.70 mol of A and 3.90 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A] = { [B] = [C] =
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc 3 A(g) 2 B(g)= 4C(g) = 1.53 x 1019 К If, at this temperature, 2.10 mol of A and 3.80 mol of B are placed in a 1.00L container, what are the concentrations of A, B, and C at equilibrium? [A] М М [B= [C] М =
At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc = 3.13 x 1027 3A(g) + 2B(g) 4C(g) If, at this temperature, 1.40 mol of A and 4.00 mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium?
At a certain temperature, the equilibrium constant, Kc , is 0.00401 for the reaction Cl2(g)−⇀↽−2Cl(g) A. If 3.05 g Cl2Cl2 is placed in a 3.00 L flask at this temperature, what are the equilibrium concentrations of Cl2 and Cl? B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 4.50 L while the temperature is held constant. What are the new equilibrium concentrations of Cl2 and Cl? C. Following the establishment of...