This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
~Mataa🫶🏽, let's knock this out. To calculate the equilibrium concentration of F6P, we need to consider the two sequential equilibrium reactions. Step 1: Calculate the equilibrium concentration of G6P from the first reaction. The first reaction is: C_6H_12O_6(aq) + ATP(aq) G6P(aq) + ADP(aq) The equilibrium constant for this reaction is K_1 = 4.63 × 10^3. The equilibrium expression is: K_1 = ([G6P][ADP])/([C_6H_12)O_6][ATP] We are given the following equilibrium concentrations: [C_6H_12O_6] = 1.2 × 10^-6 M [ATP] = 1.0 × 10^-4 M [ADP] = 1.0 × 10^-2 M Rearrange the equation to solve for [G6P]: [G6P] = K_1 × [C_6H_12O_6][ATP][ADP] Substitute the given values: [G6P] = (4.63 × 10^3) × (1.2 × 10^-6 M)(1.0 × 10^-4 M)(1.0 × 10^-2 M) [G6P] = (4.63 × 10^3) × 1.2 × 10^-101.0 × 10^-2 [G6P] = (4.63 × 10^3) × (1.2 × 10^-8) [G6P] = 5.556 × 10^-5 M Step 2: Calculate the equilibrium concentration of F6P from the second reaction. The second reaction is: G6P(aq) F6P(aq) The equilibrium constant for this reaction is K_2 = 2.76 × 10^-1. The equilibrium expression is: K_2 = ([F6P])/([G6P]) We use the equilibrium concentration of [G6P] calculated in Step 1. Rearrange the equation to solve for [F6P]: [F6P] = K_2 × [G6P] Substitute the values: [F6P] = (2.76 × 10^-1) × (5.556 × 10^-5 M) [F6P] = 1.533456 × 10^-5 M Step 3: Round the final answer to the appropriate number of significant figures. The given concentrations have 2 significant figures (1.2 × 10^-6 M, 1.0 × 10^-4 M, 1.0 × 10^-2 M). Therefore, the final answer should be rounded to 2 significant figures. [F6P] ≈ 1.5 × 10^-5 M The equilibrium concentration of F6P is 1.5 × 10^-5 M. Got more? Send 'em!