Choose the general expression for the equilibrium constant for the following reactions: Part A aA(aq) + bB(aq) =cC(aq) + dD(ag) OK. [A]*|B]" O K : %3| [A]°[B]* O K, PEPS o Kp = PRP Submit Request Answer Part B aA(g) + bB(g) =C(g) + dD(g) O K : %3D o K : PEP P O K, O K = [A]*[B]* Submit Request Answer

The reaction 4A (aq) + 6B (aq) =C (aq) + 3D (aq) is run and the measured concentrations are given in the table below. [A] [B] [C] [D] 1.43 0.74 0.56 1.10 Initial 0.70 0.36 1.35 1.80 Equilibrium What is the value of the equilibrium constant for this reaction? Please express your answer in scientific notation to the second decimal place NOTE: Please don't ICE table this guy, the numbers are randomly generated so any ICE table efforts won't work out.

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5) Determine the value of K for the following reaction if the equilibrium concentrations are as follows: [P4010leg = 4.000 moles, [P4leq = 4.000 moles, [O2leg = 2.000 M %3D %3D P4(s) + 5 02(g) P4010(s) 6) Determine the value of K for the following reaction if the equilibrium concentrations are as follows: [N2leq 2.25 M, [O2leg = 3.67 M, [N20]eg = 3.39 M. %3D %3D %3D 2 N20(g) = 2 N2(g) + 02(g)

When determining the equilibrium concentrations for the reaction AB(g) A(g) + B(g) [A][B] [AB] a simplifying assumption can be used under certain conditions to avoid solving a quadratic equation. Ke Kc = [AB]-x [AB] Classify each situation by whether the simplifying assumption can be used or whether the quadratic formula is required. Simplifying assumption can be used [AB] = 0.00178 M. Kc = 9.91 x 107 [AB]=0.0353 M, K, 3.67 x 10 Answer Bank [AB]=0.484 M, K, 8.18 x 10 Quadratic formula required [AB] 0.176 M. K=144 x 10¹ [AB]=0.0160 M, K - 7.46 x 10

The equilibrium constant, K, for the following reaction is 77.5 at 600 K CO(g) + Cl₂(g) CoCl₂(g) Calculate the equilibrium concentrations of reactant and products when 0.483 moles of CO and 0.483 moles of Cl₂ are introduced into a 1.00 L vessel at 600 K. [co] [Cl₂] [COCI,]= Submit Answer M M M Retry Entire Group 6 more group attempts remaining

Consider the reaction 2 A + B <=> 3C + D. 3.00 moles A and 2.00 moles B was placed in a 2.00 L flask and allowed to reach equilibrium. At equilibrium the concentration of D was 0.500 M. Calculate Kc for this reaction.

A mixture initially contains AA, BB, and CC in the following concentrations: [A][A] = 0.300 M� , [B][B] = 0.900 M� , and [C][C] = 0.550 M� . The following reaction occurs and equilibrium is established: A+2B⇌CA+2B⇌C At equilibrium, [A][A] = 0.150 M� and [C][C] = 0.700 M� . Calculate the value of the equilibrium constant, Kc�c. Express your answer numerically. View Available Hint(s)for Part A

2. Write the equilibrium expression as K. for the following reactions: a) (NH4)2Se(s) 2NH3(g) + H₂Se(g) b) AgCl(s) Ag*(aq) + Cl(aq) c) P4(s) +6Cl2(g) = 4PC|3(1) 1