At a certain temperature, the equilibrium constant for the following chemical equation is 2.50. SO2(g) + NO2(g)<--->...

Free

90.2K

Verified Solution

Question

Chemistry

At a certain temperature, the equilibrium constant for thefollowing chemical equation is 2.50.
SO2(g) + NO2(g)<---> SO3(g) + NO(g)
At this temperature, calculate the number of moles of NO2(g)that must be added to 2.86 mol of SO2(g) in order to form 1.30 molof SO3(g) at equilibrium.
Solve for the number of moles for NO2

Answer & Explanation Solved by verified expert

4.2 Ratings (515 Votes)

Given : Initial Moles of SO2 = 2.86

Let initial moles of NO2 = x

The chemical equilibrium is

Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â SO2(g)Â Â +Â Â Â NO2(g)Â Â Â Â ---> SO3(g) + NO(g)

Initial molesÂ Â Â Â Â Â Â Â Â 2.86Â Â Â Â Â Â Â Â Â Â Â Â Â Â xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0Â Â Â Â Â Â Â Â Â Â Â Â 0

ChangeÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â -yÂ Â Â Â Â Â Â Â Â Â Â Â Â -yÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â +yÂ Â Â Â Â Â Â Â Â Â Â +y

EquilibriumÂ Â Â Â Â Â Â 2.86-yÂ Â Â Â Â Â Â Â Â Â Â Â Â x-yÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â yÂ Â Â Â Â Â Â Â Â Â Â Â Â Â y
Given : mole sof SO3 at equilibrium = 1.30 so y = 1.30

Now Keq = [SO3][NO] / [SO2][NO2]

2.50 = 1.30 X 1.30 / (2.86-1.30) (x-1.30)

1.48 = 1 / 1.56 X (x-1.30)

(x-1.30) = 0.433

x = 1.733 moles

so number of moles of NO2 that must be added = 1.733 moles

Get Answers to Unlimited Questions

Join us to gain access to millions of questions and expert answers. Enjoy exclusive benefits tailored just for you!

Membership Benefits:

Unlimited Question Access with detailed Answers
Zin AI - 3 Million Words
10 Dall-E 3 Images
20 Plot Generations
Conversation with Dialogue Memory
No Ads, Ever!
Access to Our Best AI Platform: Flex AI - Your personal assistant for all your inquiries!

Become a Member