Express the equilibrium constant for the following reaction.

CsIO3(s) CsIO(s) + O2(g)

Question

Express the equilibrium constant for the following reaction.

CsIO3(s)  CsIO(s) + O2(g)

BlackTom AI · Accepted Answer

Question restatement: Express the equilibrium constant for the decomposition reaction CsIO3(s)  → CsIO(s) + O2(g).

First, identify which species are in the gas phase versus solids. The two solid iodates (CsIO3(s) and CsIO(s)) have activities that are defined as 1 in equilibrium expressions, so they do not appear in the numerator or denominator of the expression.

Next, write the equilibrium constant expression in terms of activities. Since only O2 is gaseous, the equilibrium constant K is determined entirely by the activity of O2: K = a(O2).

Different conventions exist depending on whether you use activities, partial pressures, or concentrations:
- If you formulate Kp (in terms of partial pressures), Kp equals the partial pressure of O2, P(O2).
- If you formulate Kc (in terms of concentrations), you would use the concentration of O2, [O2], but note that [O2] is related to P(O2) through the ideal gas law and standard state conventions, so Kc and Kp are not numerically identical unless you account for those factors.

Thus, the general statement is that the equilibrium constant is governed by the oxygen phase, and can be written as K = a(O2) = P(O2) (for gas-phase standard state of 1 bar) or, equivalently, Kc = [O2] if you are explicitly using concentrations with the appropriate standard-state conventions. In any standard chemistry treatment, the two solids do not contribute to the expression because their activities are constant and set to 1.

About the provided answer choice: saying K = [O2] is only correct if one is specifically using a concentration-based form Kc and the standard state is defined so that [O2] represents the appropriate reference concentration. More precisely and generally, the expression should be K = a(O2) or Kp = P(O2); using a simple [O2] without clarifying the form (Kc vs Kp) can be ambiguous and potentially misleading because the numeric relationship between Kc and Kp depends on the temperature and the gas constant. The key conceptual point remains: solids cancel, and the remaining dependence is on the oxygen species in the gas phase, not on CsIO3(s) or CsIO(s).

Express the equilibrium constant for the following reaction. CsIO3(s) CsIO(s) + O2(g)

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