The following reaction has a K = 0.145 2BrCl Br₂ + Cl₂ 2 If the concentrations are [BrCl] = 0.050 M, [Br2] = 0.035 M, and [Cl2] = 0.030M, Calculate Q. D

18. The equilibrium constant Ke for the reaction below is 5.0 × 104 at 25°C. Ni(s) + 4CO(g) = Ni(CO)4(g) What is the equilibrium constant for the following reaction at 25°C? 2Ni(CO)4(g) = 2Ni(s) + 8CO(g)

At a particular temperature, K = 3.68 for the reaction SO2(g) + NO2(g) = SO3(g) + NO(g) Calculate the concentrations of all four gases at equilibrium when 0.574 mol of each gas is mixed in a 1.000-L flask. (In other words, the concentration of each gas is 0.574 M.) HOW DO WE GET THERE? We will define the change in the concentrations to reach equilibrium in terms of x. Let x equal the number of moles per liter of SO, and NO, consumed to reach equilibrium. SO2(g) + NO2(g) = SO3(g) + NO(g) Initial: 0.574 0.574 0.574 0.574 Change: -X +x +x -x Equilibrium: 0.574-x 0.574-x 0.574+x 0.574+x Therefore, [SO,]]NO] [SO,]]NO,] (0.574+æ)(0.574+æ) (0.574 – x)(0.574 – x) K = 3.68 = What is the value of x? X =

Given these initial concentrations: [SCN] = 0.000646 M, [Fe³+] = 0.000506 M, and [Fe(SCN)²+] = 0.000000 M, determine The value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M. value for K: 1.09 X10-4 Incorrect

Consider the reaction:  4 A (g) + 3 B (g)   2 C (g)  +  5 E (g).   The reaction is initiated with 0.60 M in A, 0.45 M in B and 0.50 M in E.  At equilibrium, the value of  [A] = 0.36 M.  What is the equilibrium value of [E]?

How long will it take for the concentration of A to decrease from 0.910 M to 0.387 for the reaction A → Products? (k = 0.153 M/s)

Given these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] = 0.000 M, determine the value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M.

Consider the reaction N2 (9) + 02 (e) + 2NO (e) that has K= 4 x 10-6 . Initially, 0.1 M N2 and 0.1 M O2 are placed in a container. What is the equilibrium concentration of NO? O 2.0 x 102 M O 1.4 x 102 M O 2.0 x 10-4 M O 1.0 x 10-4 M O 4.0 x 10-4 M

How long will it take for the concentration of A to decrease from 0.910 M to 0.573 for the reaction A → Products? (k = 0.153 M/s)