Find The Value Of Ax B 3x C6x H - Gauthmath

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SHOW LESS116

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Answer# Answer K_eq equals StartFraction StartBracket upper C EndBracket StartBracket upper D EndBracket over StartBracket upper A EndBracket StartBracket upper B EndBracket EndFraction.Explanation# Explanation The equilibrium constant expression for a reversible reaction is based on the law of mass action. It states that at equilibrium, the ratio of the products of the concentrations of the products raised to the power of their coefficients to the products of the concentrations of the reactants raised to the power of their coefficients is constant. For the given general reaction: \[ aA + bB \rightleftharpoons cC + dD \] The equilibrium constant expression, \( K_{eq} \), is given by: \[ K_{eq} = \frac{[C]^c[D]^d}{[A]^a[B]^b} \] where: - \( [A] \), \( [B] \), \( [C] \), and \( [D] \) represent the molar concentrations of the reactants and products at equilibrium. - \( a \), \( b \), \( c \), and \( d \) represent the stoichiometric coefficients of the reactants and products in the balanced chemical equation. ### Step 1 Identify the reactants and products along with their stoichiometric coefficients from the given reaction. In this case, the coefficients are not given, so we assume them to be 1 for each reactant and product. ### Step 2 Write the equilibrium constant expression by placing the concentrations of the products in the numerator and the concentrations of the reactants in the denominator. Each concentration is raised to the power of its respective stoichiometric coefficient. ### Step 3 Since the coefficients are assumed to be 1 (as they are not specified), the equilibrium constant expression simplifies to the concentrations without exponents.Click to rate:88.3(618 votes)Search questionBy textBy image/screenshotDrop your file here orClick Hereto upload