To find the standard reduction potential (E⊖) for the reaction Cr+2+2e−→Cr, we can use the given reduction potentials for the reactions E⊖forCr3++3e−→Cr (-0.74V) and Cr3++e−→Cr2+ (-0.40V).

Step 1: Write the balanced equation for the reaction we are interested in:
Cr+2 + 2e− → Cr

Step 2: Identify the half-reactions involved in the reaction:
Half-reaction 1: Cr3+ + 3e− → Cr (E⊖ = -0.74V)
Half-reaction 2: Cr3+ + e− → Cr2+ (E⊖ = -0.40V)

Step 3: Determine the reduction potential for the desired reaction:
Since the reduction potential is a measure of the tendency of a species to gain electrons, we can subtract the reduction potential of the oxidation half-reaction from the reduction potential of the reduction half-reaction to obtain the reduction potential for the desired reaction.

E⊖ for the reaction = E⊖ reduction - E⊖ oxidation
E⊖ for the reaction = (-0.40V) - (-0.74V)
E⊖ for the reaction = 0.34V

Therefore, the standard reduction potential (E⊖) for the reaction Cr+2+2e−→Cr is 0.34V.

Question

To find the standard reduction potential (E⊖) for the reaction Cr+2+2e−→Cr, we can use the given reduction potentials for the reactions E⊖forCr3++3e−→Cr (-0.74V) and Cr3++e−→Cr2+ (-0.40V).

Step 1: Write the balanced equation for the reaction we are interested in:
Cr+2 + 2e− → Cr

Step 2: Identify the half-reactions involved in the reaction:
Half-reaction 1: Cr3+ + 3e− → Cr (E⊖ = -0.74V)
Half-reaction 2: Cr3+ + e− → Cr2+ (E⊖ = -0.40V)

Step 3: Determine the reduction potential for the desired reaction:
Since the reduction potential is a measure of the tendency of a species to gain electrons, we can subtract the reduction potential of the oxidation half-reaction from the reduction potential of the reduction half-reaction to obtain the reduction potential for the desired reaction.

E⊖ for the reaction = E⊖ reduction - E⊖ oxidation
E⊖ for the reaction = (-0.40V) - (-0.74V)
E⊖ for the reaction = 0.34V

Therefore, the standard reduction potential (E⊖) for the reaction Cr+2+2e−→Cr is 0.34V.

Knowee AI · Accepted Answer

To find the standard reduction potential (E⊖) for the reaction Cr+2+2e−→Cr, we can use the given reduction potentials for the reactions E⊖forCr3++3e−→Cr (-0.74V) and Cr3++e−→Cr2+ (-0.40V).

Step 1: Write the balanced equation for the reaction we are interested in:
Cr+2 + 2e− → Cr

Step 2: Identify the half-reactions involved in the reaction:
Half-reaction 1: Cr3+ + 3e− → Cr (E⊖ = -0.74V)
Half-reaction 2: Cr3+ + e− → Cr2+ (E⊖ = -0.40V)

Step 3: Determine the reduction potential for the desired reaction:
Since the reduction potential is a measure of the tendency of a species to gain electrons, we can subtract the reduction potential of the oxidation half-reaction from the reduction potential of the reduction half-reaction to obtain the reduction potential for the desired reaction.

E⊖ for the reaction = E⊖ reduction - E⊖ oxidation
E⊖ for the reaction = (-0.40V) - (-0.74V)
E⊖ for the reaction = 0.34V

Therefore, the standard reduction potential (E⊖) for the reaction Cr+2+2e−→Cr is 0.34V.

E⊖forCr3++3e−→Cr and Cr3++e−→Cr2+ are −0.74V and −0.40V, respectively. E⊖ for the reaction is: Cr+2+2e−→Cr

Question

E⊖ for the reaction $\text{Cr}^{2+} + 2e^{-} \rightarrow \text{Cr}$ is:

Solution

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