A voltaic cell consists of a standard hydrogen electrode and a second half-cell in which a magnesium electrode is immersed in a 1.00 M solution of Mg2+ ions. Calculate Ecell given that the standard reduction potential for the magnesium half-reaction is -2.37 V.

The correct answer is "+2.37 V".

Explanation:

Given that,

Concentration of

= 1.00 M

,

= -2.37 V

,

= 0.00V

When S.H.E as well as anode act as cathode, then

⇒

By putting the values, we get

⇒            

⇒                

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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