Using the dissociation constant, Kd = 2.2x10^-34, calculate the equilibrium concentrations of Co3 and NH3 in a 0.500-M solution of Co(NH3)6^3.
Using the dissociation constant, Kd = 2.2x10^-34, calculate the equilibrium concentrations of Co3 and NH3 in...
The acid dissociation constant Ka of trichloroacetic acid CCl3COOH, is 2.2x10^-1 calculate the ph of 1.00 M aqueous solution of trichloroacetic acid.
Calculate the equilibrium concentration of Co3+ (aq) in a solution that is initially 0.0300 M CO(NO3)2 and 0.500M NH3. The formation constant for CO(NH3)6]** (aq) is Kf= 2.3 x 1033 ICO(NL) I Costa
12. Calculate the equilibrium constant for the following reaction if the equilibrium concentrations of NH3, N2, and H, are 0.0100 M, 0.100 M, and 0.162 M, respectively. 2NH, (g) N2(g) + 3H2(8)
Calculate the equilibrium constant for the reaction using the balanced chemical equation and the concentrations of the substances at equilibrium. Use the appropriate significant figures in reporting the answers. CO(g) + H2O(g) ⇌ CO2(g) + H2(g) [CO] = 0.0590 M; [H2O] = 0.00600 M; [CO2] = 0.0410 M; [H2] = 0.0410 M K =
At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction Part A aA +bB = C+ dD A mixture initially contains A, B, and C in the following concentrations: [A] = 0.500 M , [B] = 1.35 M , and [C] = 0.500 M. The following reaction occurs and equilibrium is established: where a, b, c, and d are...
At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction aA+bB?cC+dD where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is Kc=[C]c[D]d[A]a[B]b where [A], [B], [C], and [D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qc, instead of...
Question #9 Release kinetics. The dissociation constant KD for the release of oxygen from oxymyoglobin is 10-6 M, where the KD = [Mb][O2]/[MbO2], the rate constant for the combination of O2 with myoglobin is 2 x 107 M-1s-1. a) What is the rate constant for the dissociation of O2 from myoglobin? b) What is the mean duration of the oxymyoglobin complex?
2. For the acid dissociation reaction below, the equilibrium concentrations are given as [H'] = 0.0060 M, [C2H302] =0.0060 M and the equilibrium constant, K is given as 1.8 x10-5. HC2H3O2 (aq) + (aq) + C2H:O2 (aq) a) Write the equilibrium constant expression for the reaction b) Calculate the concentration of HC2H302 at equilibrium
a and b please 2. The equilibrium constant for the dissociation of Ag,CO, (s) + 2 Ag+ + CO; ? is K.-8.1 x 10-12 at 25°C. a) Calculate AG for the reaction when (Agt) = 1.0 x 102 M and [CO, ) = 1.0 X 10M. (4pts) Ans: Ans: b) (1pt) Is the reaction spontaneous or nonspontaneous at these concentrations?
calculate the concentration of Co3+ om solution when 40.0 ml of 0.010 M Co(NO3)3 aq is mixed with 10.0 ml of 6.00 M NH3 aq given Co3+(aq) + 6NH3(aq) = (Co(NH3)6)3+(aq) Kf=4.5 x 10 (33)