Help Write an equilibrium constant expression for each of the following reactions. If gases are involved, write the expression in terms of partial pressures.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3)2 as (P NH3)2. If either the numerator or denominator is 1, please enter 1.(a)(b)(c)(d)COCI₂(g) ← CO(g) + Cl₂(9)Kp2 MnO₂ (s)Kp =2 MnO(s) + O₂(g)PbCl₂(s) ← Pb²+ (aq) + 2 CI (aq)C6H14(1) ← C6H14 (9)Kp = Given that K₁ and K₂ are the respective equilibrium constants for the two reactionsMnO₂ (s) + 2H₂(g) ? Mn(s) + 2H₂O(1)CO₂(g) + H₂(9) ? CO(g) + H₂O(1)K₁= = 40.8K₂== 3.08x10-4Determine the equilibrium constant for the reactionMn(s) + 2 CO₂(g) 2 MnO₂ (s) + 2 CO(g) K =

To write the expression of equilibrium constant, general formula is : K= ProductsReactants While…

Write an equilibrium constant expression for each of the following reactions. If gases are involved, write the expression in terms of partial pressures. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH₂)2 as (P NH3)2. If either the numerator or denominator is 1, please ente (a) (b) (c) (d) COCI₂ (9) → CO(g) + Cl₂(9) Kp 2 MnO₂ (s) Kp = PbCl₂(s) → Pb²+ (aq) + 2 Cl(aq) C6H14(1) Kp 2 MnO(s) + O₂(g) = C6H14 (9)