In the equilibrium described in Example 15-12, the percent dissociation of N 2 O 4 can be

Question:

In the equilibrium described in Example 15-12, the percent dissociation of N2O4 can be expressed as

3.00 x 103 mol N204 0.0240 mol NO4 initially X 100% = 12.5%

What must be the total pressure of the gaseous mixture if N2O4(g) is to be 10.0% dissociated at 298 K?

N2O4 2 NO(g) Kp = 0.113 at 298 K

(for pressures in atmospheres).


Example 15-12

A 0.0240 mol sample of N2O4(g) is allowed to come to equilibrium with NO2(g) in a 0.372 L flask at 25 °C. Calculate the amount of N2O4 present at equilibrium (Fig. 15-9).

NO4(g) 2 NO(g) Kc = 4.61 x 10 at 25 C

Figure 15-9

& og 88 88 88 (a) 88 &g 8 88 = NO4 = NO S88 (b)

Fantastic news! We've Found the answer you've been seeking!

Step by Step Answer:

Related Book For  book-img-for-question

General Chemistry Principles And Modern Applications

ISBN: 9780132931281

11th Edition

Authors: Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette

Question Posted: