-Print Calculator Periodic Print Calculator -d Periodic Table Question 12 of 26

Question

-Print Calculator Periodic Print Calculator -d Periodic Table Question 12 of 26 Phosphorus pentachloride decomposes according to the chemical equation Map ot =1.80 at 250°C A 0.294 mol sample of PCIs(g) is injected into an empty 3.80 L reaction vessel held at 250 . Calculate the concentrations of PC(g) and PCl3(g) at equilibrium Number [PC15] = Number O Previous Give up & View Solution e Check Answer O Next Exit Start by finding the initial concentration of PCls from the number of moles and the volume. Then, set up a table of initial and final concentrations, where the change in concentration of each product is designated as x.

Explanation / Answer

Solution :-

Given data

0.294 mol PCl5

Volume = 3.80 L

Kc =1.80

PCl5(g)------ > PCl3(g) + Cl2(g)

Equilibrium concentration of the PCl5and PCl3 = ?

Lets first calculate the initial molarity of the PCl5

Molarity of PCl5 = 0.294 mol / 3.80 L

= 0.07737 M

Now lets set up the ICE table

PCl5(g)------ >PCl3(g)+Cl2(g

0.07737 M      0           0

-x                  +x         +x

0.07737-x        x           x

Lets write the equilibrium constant equation

Kc =[PCl3][Cl2]/[PCl5]

Lets put the values in the formula

1.80 = [x][x]/[0.07737-x]

1.80* (0.07737-x)= x^2

0.13927 -1.80x =x^2

Solving this using the quadratic equation we get

X= 0.07430 M

Therefore the equilibrium concentration of the PCl5 is as follows

[PCl5] = 0.07737-x

= 0.07737 – 0.07430

= 0.00307 M

And equilibrium concentration of the PCl3 =x = 0.07430 M

Related Questions

Navigate

• Browse (All)
• Browse #
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.