Crowdly

Add to Chrome

CHEM 1023 WI01-04 General Chemistry 2 2025 Winter

Looking for CHEM 1023 WI01-04 General Chemistry 2 2025 Winter test answers and solutions? Browse our comprehensive collection of verified answers for CHEM 1023 WI01-04 General Chemistry 2 2025 Winter at moodle.acadiau.ca.

Get instant access to accurate answers and detailed explanations for your course questions. Our community-driven platform helps students succeed!

F=96485 C mol^-1, R=8.314 J mol^-1K^-1, T=298 K

Part A

Using the table below, calculate the equilibrium constant for the electrochemical cell represented by the following line notation:

Cr(s)|Cr³⁺(aq)||Fe²⁺(aq)|Fe(s)

Express your answer to two significant figures.

Part B

For the reaction above, calculate the standard Gibbs energy change.

Write your answer to three significant figures.

Δ_rG° =

kJ/mol

Part C

Based on your answer in Part B, identify the spontaneity of the reaction:

The above redox reaction is

spontaneous.

non-spontaneous

at equilibrium

Standard Electrode Potentials at 25ºC Eº(V)

Ag⁺(aq)+e⁻	→Ag(s)	0.80
Pb²⁺(aq)+2e⁻	→Pb(s)	-0.13
Ni²⁺(aq)+2e⁻	→Ni(s)	-0.23
Co²⁺(aq)+2e⁻	→Co(s)	-0.28
Cd²⁺(aq)+2e⁻	→Cd(s)	-0.40
Fe²⁺(aq)+2e⁻	→Fe(s)	-0.45
Cr³⁺(aq)+3e⁻	→Cr(s)	-0.73
Zn²⁺(aq)+2e⁻	→Zn(s)	-0.76
Mn²⁺(aq)+2e⁻	→Mn(s)	-1.18
Al³⁺(aq)+3e⁻	→Al(s)	-1.66

View this question

The standard reduction potentials of lithium metal and chlorine gas are as follows:

Li⁺(aq) + e⁻→ Li(s) E°

=−3.04 V

Cl₂(g) + 2e⁻→ 2Cl⁻(aq) E°=

+1.36 V

Part A

Calculate the cell potential of a galvanic cell involving the half-reactions shown above under standard conditions.

Express your answer to two decimal places.

E°_cell =

Part B

Calculate the standard Gibbs energy change

of the reaction.

Express your answer to three significant figures.

Δ_rG° = kJ/mol

View this question

Which species can oxidize Cd

but not Sn?

A table of standard electrode potentials is available on Moodle.

View this question

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Sn²⁺(aq) + 2e^– → Sn(s) E° = -0.14 V

Zn²⁺(aq) + 2e^– → Zn(s)

E° = -0.76 V

Mn²⁺(aq) + 2e^– → Mn(s) E° = –1.18 V

View this question

Part A

Using the table below, calculate the standard cell potential for the following reaction:

Zn(s)+2Ag⁺(aq

)→Zn²⁺(aq)+2Ag(s)

Express your answer to two decimal places.

Eº_cell = V

Part B

Determine whether or not the cell reaction above is spontaneous as written, under standard conditions:

non-spontaneous

spontaneous

Standard Electrode Potentials at 25^ºC Eº (V)

Ag⁺(aq)+e⁻	→Ag(s)	0.80
Pb²⁺(aq)+2e⁻	→Pb(s)	-0.13
Ni²⁺(aq)+2e⁻	→Ni(s)	-0.23
Co²⁺(aq)+2e⁻	→Co(s)	-0.28
Cd²⁺(aq)+2e⁻	→Cd(s)	-0.40
Fe²⁺(aq)+2e⁻	→Fe(s)	-0.45
Cr³⁺(aq)+3e⁻	→Cr(s)	-0.73
Zn²⁺(aq)+2e⁻	→Zn(s)	-0.76
Mn²⁺(aq)+2e⁻	→Mn(s)	-1.18
Al³⁺(aq)+3e⁻	→Al(s)	-1.66