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A homogeneous equilibrium is one in which all species are present in the same phase. Common examples include gas-phase or solution reactions. A heterogeneous equilibrium is one in which species exist in more than one phase. Common examples include reactions involving solids and gases, or solids and liquids. Compare this with the chemical equation for the equilibrium. The convention is that the substances on the right side of the equation are written in the numerator of the Kc expression, and those on the left side in the denominator. The exponents are the coefficients of the reactants and products from the equation. It is helpful to write down the chemical equation for a equilibrium reaction whenever discussing an equilibrium constant, to ensure the expression is written correctly (products over reactants). Both the copper on the left-hand side and the silver on the right are solids. Both are left out of the equilibrium constant expression: