Calculate a value for the equilibrium constant for the reactionO₂(g) + O(g) → 03 (9)givenhv-49NO₂(g) → NO(g) + O(g) K = 7.3 × 10-O3 (9) + NO(g) ⇒ NO₂(g) + O2(g) K = 5.9 × 10-³4(Hint: When reactions are added together, the equilibrium expressions are multiplied.)K= At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide:N2 (9) + O2(g) ⇒ 2 NO(g)= 0.077 M, andSuppose the system is analyzed at a particular temperature, and the equilibrium concentrations are found to be [N₂] = 0.050 M, [O₂] =[NO] = 6.3 × 10-4 M. Calculate the value of K for the reaction.K = 1.0x10^-5

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Calculate a value for the equilibrium constant for the reaction
O₂(g) + O(g) → 03 (9)
given
hv
-49
NO₂(g) → NO(g) + O(g) K = 7.3 × 10-
O3 (9) + NO(g) ⇒ NO₂(g) + O2(g) K = 5.9 × 10-³4
(Hint: When reactions are added together, the equilibrium expressions are multiplied.)
K=

At high temperatures, elemental nitrogen and oxygen react with each other to form nitrogen monoxide:
N2 (9) + O2(g) ⇒ 2 NO(g)
= 0.077 M, and
Suppose the system is analyzed at a particular temperature, and the equilibrium concentrations are found to be [N₂] = 0.050 M, [O₂] =
[NO] = 6.3 × 10-4 M. Calculate the value of K for the reaction.
K = 1.0x10^-5

Expert Solution

Step 1: Equilibrium constant

Equilibrium constant K for a reaction is defined as the product of the molar concentrations of the products, each raised to the power equal to a stoichiometric coefficient divided by the product of the molar concentrations of the reactant each raised to the power equal to its stoichiometric coefficient .
& the most important convention to be kept in mind is that the active mass of a pure solid or pure liquid is considered to be constant.

Characteristics of equilibrium constant are : -

If the equation having equilibrium constant K is written into steps having equilibrium constant K1 and K2 then K1 * K2 = K .

If the reaction is reversed, the value of the equilibrium constant is inversed.

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