Constants Periodic Table Part A The reversible chemical reaction A+B C+ D Initia

Question

Constants Periodic Table Part A The reversible chemical reaction A+B C+ D Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached? has the following equilibrium constant: Express your answer to two significant figures and include the appropriate units. View Available Hint(s) alue Submit V Part B 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 View Available Hint(s) [D] | Value Submit

Explanation / Answer

Answer: [A]=0.54 M

Explanation: The "REVERSIBLE" chemical reaction-
A + B <--> C + D
Kc = [C][D] / [A][B] = 7.2
Concentration at the start and after equilibrium-
[A] = 2.00 M --> (2.00 - X) M
[B] = 2.00 M --> (2.00 - X) M
[C] = 0.00 M --> X M
[D] = 0.00 M --> X M
7.2 = X^2 / (2.00 - X)^2
take the square root of both sides-
2.68 = X / (2.00 - X)
5.36 - 2.68 X = X
5.36 = 3.68 X
X = 1.46
at equilibrium-
[A] = 0.54 M
[B] = 0.54 M
[C] = 1.46 M
[D] = 1.46 M

Part 2:
7.2 = X^2 /{(1.00 - X)(2.00 - X)}  
6.2X^2 -21.6X +14.4 = 0
X = 0.898
[D] = 0.90 M

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