12/5/2016 11:00 PM A 61.8/100 11/29/2016 10:09 AM Gradebook Print calculator Per

Question

12/5/2016 11:00 PM A 61.8/100 11/29/2016 10:09 AM Gradebook Print calculator Periodic Table Question 10 of 27 Map University Science Books General Chemistry 4th Edition McQuarrie Rock Gallogl presented by Sapling Learning At a certain temperature, the equilibrium constant for the following chemical equation is 2.10. so g) NO2 (g) so, (g) Nolg) At this temperature, calculate the number of moles of NO2(g) that must be added to 2.99 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium. Number mol of NO 2(g) Previous ® Give Up & View Solution Check Answer Next Exit Hint

Explanation / Answer

Let the number of moles of NO2 be n

SO2 (g) + NO2 (g) <---------> SO3 (g) + NO (g)
2.99 n 0 0 (initial)
2.99-x n-x x x (at equilibrium)

here x = 1.3 mol

K = x*x / {(2.99-x)*(n-x)}
2.10 = 1.3*1.3 / {(2.99-1.3)*(n-1.3)}
2.10 = 1.69 / (1.69*(n-1.3))
n-1.3 = 0.48
n = 1.78

Answer: 1.78 mol of NO2

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

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