11 Consider the following equilibrium CO2(g) CF4(g) 2 COF2(g) (6 pts) (a). A mix

Question

11 Consider the following equilibrium CO2(g) CF4(g) 2 COF2(g) (6 pts) (a). A mixture of CO2 and CF is prepared in a 2.00-L flask, heated to 1000°C, and allowed to come to equilibrium. Once equilibrium is reached, the flask is found to contain 0.4212 g CO2, 0.8424 g CF4, and 0A468 g COF2. Find the numerical value of equilibrium constant for the above reaction at the temperature of this experiment. (10 pts) (b). Now suppose that an additional 0.2000 g of COF2 is added to the equilibrium mixture above and the system is allowed to return to equilibrium. What will be the final concentration of COF2 once equilibrium is restored?

Explanation / Answer

Step 1: Convert the mass to moles.

0,4212 g CO2 x (1 mol CO2/44,01 g CO2) = 9,57 x 10-3 moles CO2

0,8424 g CF4 x (1 mol CF4/88,00 g CF4) = 9,57 x 10-3 moles CF4

0,4468 g COF2 x (1 mol COF2/88,00 g COF2) = 9,57 x 10-3 moles COF2

Step 2: Convert moles to molarity (mol/L)

9,57 x 10-3 moles CO2 / 2,00 L = 4,78 x 10-3 M CO2

9,57 x 10-3 moles CF4 / 2,00 L = 4,78 x 10-3 M CF4

6,77 x 10-3 moles COF4 / 2,00 L = 3,38 x 10-3 M COF4

Step 3: Calculate the equilibrium constant:

K = [COF4]2/[CO2][CF4]

K = (3,38 x 10-3 M)2/(4,78 x 10-3 M)(4,78 x 10-3 M)

K = 1,14 x 10-5

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