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…

Answered: Write an equilibrium constant…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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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)
Kp
2 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 reactions
MnO₂ (s) + 2H₂(g) ? Mn(s) + 2H₂O(1)
CO₂(g) + H₂(9) ? CO(g) + H₂O(1)
K₁= = 40.8
K₂=
= 3.08x10-4
Determine the equilibrium constant for the reaction
Mn(s) + 2 CO₂(g) 2 MnO₂ (s) + 2 CO(g) K =

Expert Solution

Step 1

To write the expression of equilibrium constant, general formula is :

$K = \frac{P r o d u c t s}{R e a c \tan t s}$

While write the expression, only solid and aqueous species are considered . Solid and liquid compounds are not considered because their concentration is assumed to be constant throughout the reaction.

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