1
answer
0
watching
485
views
19 Nov 2019

Given
N2(g) + O2(g) ↔ 2NO(g) Kc1 = 1.0 x 10-30
N2(g) + Br2(g) + O2(g) ↔ 2NOBr(g) Kc2 = 2.0 x 10-27

(a) What is the Kc for the reaction: 2NO(g) + Br2(g) ↔ 2NOBr (g)? ΔHo = – 47.14 kJ

(b) If you start with [NO] = 5.0 x10-3 M, [Br2] = 1.9 x 10-3 M, and [NOBr] = 6.9 x 10-3 M, is the reaction at equilibrium? If not, predict the direction in which reaction will occur to reach equilibrium.

(c) What is the ΔGo and ΔSo of the above reaction? Is the reaction spontaneous or nonspontaneous at 25oC

(d) At what temperature in oC the spontaneity of the above reaction will shift? (i.e. spontaneous becomes non-spontaneous or vice versa)

For unlimited access to Homework Help, a Homework+ subscription is required.

Nestor Rutherford
Nestor RutherfordLv2
11 Apr 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Related questions

Weekly leaderboard

Start filling in the gaps now
Log in