The reversible chemical reaction A + B C + D) has the following equilibrium cons

Question

The reversible chemical reaction A + B C + D) has the following equilibrium constant: Kc = [C][D] / [A][B] = 5.6 Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units. [A] = What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M? Express your answer to two significant figures and include the appropriate units. [D] =

Explanation / Answer

x*x/(2-x)^2 = 5.6 x = 2.36 [2-x] 4.73 /3.36 = x = 1.408 2 - 1.408 = 0.59 m answer !!! b) x*x/(1-x)(2-x) = 5.6 x*X = 5.6 [ x*x -3x + 2 ] 4.6 x*x - 16.8x + 11.2 = 0 x = 16.8 - [282.24 - 206.08] / 9.2 : x = 0 .87 answer !!!

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