Express the equilibrium constant for the following reaction.

10 PCl5(g) 10 PCl3(g) + 10 Cl2(g)

Question

Express the equilibrium constant for the following reaction.

10 PCl5(g)  10 PCl3(g) + 10 Cl2(g)

BlackTom AI · Accepted Answer

To express the equilibrium constant for the given reaction, we first identify the balanced equation and the stoichiometric coefficients. The reaction is: 10 PCl5(g) ⇌ 10 PCl3(g) + 10 Cl2(g).

Next, apply the general form of the equilibrium constant expression for a gas-phase reaction using activities (approximated by concentrations or partial pressures). For this reaction, the expression is the product of the activities of the products each raised to their stoichiometric powers, divided by the product of the activities of the reactants each raised to their stoichiometric powers:

K = (a[PCl3])^10 × (a[Cl2])^10 ÷ (a[PCl5])^10.

If we are using molar concentrations (typical for Kc) or partial pressures (typical for Kp), the same structure holds. Writing it compactly, you can factor out the exponent: K = ([PCl3]^10 [Cl2]^10)/([PCl5]^10).

Equivalently, this can be written as K = ([PCl3][Cl2]/[PCl5])^10, which emphasizes that the ratio inside the parentheses is raised to the tenth power due to the 10 moles of each species involved.

Notes:
- If the problem uses Kp instead of Kc, replace concentrations with partial pressures in the same mathematical form.
- No numerical value for K is given here because the problem asks for the expression, not a computed number.
- If the provided options in a typical multiple-choice setup were present, you would choose the option that matches K = ([PCl3]^10 [Cl2]^10)/([PCl5]^10) (or its simplified power form) and reject any form that does not correspond to the correct stoichiometric exponents.

Express the equilibrium constant for the following reaction. 10 PCl5(g) 10 PCl3(g) + 10 Cl2(g)

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