🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
Chemistry
2
answers
0
watching
308
views

Forthe following reaction at equilibrium, which change will cause theequilibrium to shift to the left?

2NOBr(g)<-->2NO(g) + Br2(g),

  1. A) Increasethe container volume.

  2. B) Removesome NO.

  3. C) Removesome Br2.

  4. D) Addmore NOBr.

  5. E) Decreasethe temperature.

?Horxn= 30kJ/mol

Watch
2
answers
0
watching
308
views

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

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
Beverley Smith
Beverley SmithLv2
28 Sep 2019
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Nitrosyl bromide, NOBr, is formed in the reaction of nitric oxide,NO, with bromine,Br2 : 2NO(g)+Br(g)<---->2NOBr(g) Thereaction rapidly establishes equilibrium when the reactants aremixed. At a certain temperature the concentration of was 0.400M andthat of Br2 was 0.255M . At equilibrium the concentration of NOBrwas found to be 0.250M . What is the value of Kc at thistemperature?

An evacuated 1.000 L flask was filled at room temperature with 4.920E-2 mol NO (nitrogen monoxide) and 7.74E-3 mol Br2 (bromine). The temperature was then raised to 50.5°C, and these substances reacted to give nitrosyl bromide, NOBr:

2NO(g) + Br(g) <--> 2NOBr(g)

When equilibrium was achieved, the pressure of the gases in the flask was found to be 1.315 atm.

(a) What was the total moles of gases in the flask at equilibrium? ntotal = mol
(b) How many moles of nitrosyl bromide were formed? What was the moles of each substance in the flask at equilibrium? n(NO) = mol

n(Br2) = mol

n(NOBr) = mol
(c) What are the partial pressures of the different gases in this equilibrium mixture? p(NO) = atm

p(Br2) = atm

p(NOBr) = atm
(d) What is Kp at this temperature? Kp =

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)

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in