Log in
Chemistry
1
answer
0
watching
80
views
13 Dec 2019

If a voltaic cell has a standard cell potential, E°cell, of –1.17 V at 25 °C, what must be true of the reaction at this temperature? (select all that apply)

A. K > 1
B. K < 1
C. ?G° > 0
D. ?G° < 0
E. A reaction at standard state conditions will be spontaneous in the forward direction.
F. A reaction at standard state conditions will be spontaneous in the reverse direction.

Watch
1
answer
0
watching
80
views

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

Hubert Koch
Hubert KochLv2
17 Dec 2019

Unlock all answers

Get 1 free homework help answer.
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

The standard cell potential, E°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Calculate the standard free energy change, ΔG°, in kJ for this reaction and determine if it is spontaneous or nonspontaneous at 25°C.

The standard cell potential, E°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Calculate the standard free energy change, ΔG°, in kJ for this reaction and determine if it is spontaneous or nonspontaneous at 25°C.

−2.57 × 102 kJ, nonspontaneous
−1.28 × 102 kJ, spontaneous
−2.57 × 102 kJ, spontaneous
+2.57 × 102 kJ, nonspontaneous

In thermodynamics, we determine the spontaneity of a reaction by the sign of ΔG. In electrochemistry, spontaneity is determined by the sign of E∘cell. The values of ΔG and E∘cell are related by the following formula: ΔG∘=−nFE∘cell where n is the number of moles of electrons transferred and F=96,500J/V⋠mol e− is the Faraday constant.

Part A The standard reduction potentials of lithium metal and chlorine gas are as follows: Reaction, Reduction potential (V) Li+(aq)+e−→Li(s) −3.04

Cl2(g)+2e−→2Cl−(aq) +1.36

In a galvanic cell, the two half-reactions combine to 2Li(s)+Cl2(g)→2Li+(aq)+2Cl−(aq) Calculate the cell potential of this reaction under standard reaction conditions. Express your answer with the appropriate units.

Part B: Calculate the free energy ΔG∘ of the reaction. Express your answer with the appropriate units.

Part C:

What can be said about the spontaneity of this reaction?

The reaction is:

a. spontaneous as written.
b. spontaneous in the reverse direction.
c. at equilibrium.
d. nonspontaneous in either direction.

Which statement describes the reaction shown below under standard pressure conditions at 25 ºC?

 

A. Spontaneous forward

B. Spontaneous reverse

C. At Equilibrium

ΔGº = -70.54 kJ

ΔHº = -114.14 kJ

ΔSº = -146.43 J/K

At what temperature (in ºC) will the reaction change the direction in which it is spontaneous under standard pressure conditions?

Weekly leaderboard

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