For the reaction below, Kc = 0.60 at 550 K. The reaction starts with a 0.050 M concentration of A₂B2, at 550 K. A,B, (g) = 2 AB (g) You must use the quadratic formula to determine the equilibrium concentrations of each species. What is the equilibrium concentration of [A₂B2leq? 0.0396 M 0.0302 M 0.0213 M 0.0104 M

Using the equilibrium concentrations provided, what is the equilibrium constant for the following reaction? 203(g) = 30,(g) Substance Concentration / M O3 3.34 x 104 O2 7.56 x 101 Oa. 3.40 x 103 Ob. 3.87 х 105 Oc. 2.26 x 103 Od. 2.58 x 107 Oe. 4.42 x 10-4

Can you please explain to me how to do it?

At a certain temperature K = 1.1 x 10³ for the following reaction: Fe³+ (aq) + SCN¯(aq) ⇒ Fe(SCN)²+(aq) a) Calculate the concentration of all species at equilibrium if 0.020 moles of Fe(NO3)3 is added to 1.0 L of 0.10 M KSCN (assume no change in volume upon addition). b) After equilibrium has been reached in part a, an additional 0.0050 moles of Fe(NO3)2(SCN) is added to solution. Calculate the new equilibrium concentrations of all species assuming no change in volume.