At a certain temperature, the equilibrium constant for the following chemical eq

Question

At a certain temperature, the equilibrium constant for the following chemical equation is 2.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.20 mol of SO3(g) at equilibrium.

o 10/30/2017 1 1:00 PM 0 1 1.2/20 10/29/2017 08:50 PM -Print Calculator -d Periodic Table Gradebook Question 12 of 23 Map Sapling Learning macmilan At a certain temperature, 0.720 mol of SO3 is placed in a 1.50-L container. 2503 g) -25(),(g) +02 At equilibrium, 0.190 mol of O2 is present. Calculate Kc Number Previous e Check Answer Next Exit Hint

Explanation / Answer

initial concentration of SO3 = mol of SO3 / volume

= 0.720 mol / 1.50 L

= 0.480 M

equilibrium concentration of O2 = mol of O2 / volume

= 0.190 mol / 1.50 L

= 0.127 M

Let's prepare the ICE table

[SO3] [SO2] [O2]

initial 0.48 0 0

change -2x +2x +1x

equilibrium 0.48-2x +2x +1x

To find x, we will use the equilibrium concentration provided in the question

[O2] = 0.127

x = 0.127

Equilibrium constant expression is

Kc = [SO2]^2*[O2]/[SO3]^2

Kc = (2x)^2*(x)/(0.48-2x)^2

Kc = (2*0.127)^2*(0.127)/(0.48-2*0.127)^2

Kc = 0.160

Answer: 0.160

Feel free to comment below if you have any doubts or if this answer do not work

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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