The standard Gibbs energy for the given cell reaction in k J m o l - 1 at 298 K is: Z n s + C u 2 + a q ⟶ Z n 2 + a q + C u ( s ) , E 0 = 2 V a t 298 K ( F a r a d a y ' s c o n s t a n t , F = 96000 C m o l - 1 )

Question

The standard Gibbs energy for the given cell reaction in k J m o l - 1 at 298 K is: Z n s + C u 2 + a q &#10230; Z n 2 + a q + C u ( s ) , E 0 = 2 V a t 298 K ( F a r a d a y ' s c o n s t a n t , F = 96000 C m o l - 1 )

Quantrex Academy · Accepted Answer

Correct answer: D. - 384

For the reaction, C u 2 + a q + Z n s &#10230; Z n 2 + a q + C u s n = 2 , two electrons are exchanged &#8710; G o = - n F E o = - 2 &#215; 96000 &#215; 2 = - 384000 = - 384 &#160; k J

The standard Gibbs energy for the given cell reaction in k J m o l - 1 at 298 K is: Z n s + C u 2 + a q ⟶ Z n 2 + a q + C u ( s ) , E 0 = 2 V a t 298 K ( F a r a d a y ' s c o n s t a n t , F = 96000 C m o l - 1 )

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The standard Gibbs energy for the given cell reaction in k J m o l - 1 at 298 K is: Z n s + C u 2 + a q &#10230; Z n 2 + a q + C u ( s ) , E 0 = 2 V a t 298 K ( F a r a d a y &#39; s c o n s t a n t , F = 96000 C m o l - 1 )

Options

Correct answer

Step-by-step solution

More from Electrochemistry

The standard Gibbs energy for the given cell reaction in k J m o l - 1 at 298 K is: Z n s + C u 2 + a q ⟶ Z n 2 + a q + C u ( s ) , E 0 = 2 V a t 298 K ( F a r a d a y ' s c o n s t a n t , F = 96000 C m o l - 1 )