The standard Gibbs energy change ($\Delta G^\circ$) is related to the standard cell potential (E$^\circ$) by:
\[ \Delta G^\circ = -nFE^\circ \]
where:
n is the number of moles of electrons transferred in the balanced redox reaction.
F is Faraday's constant (96487 C mol$^{-1}$).
E$^\circ$ is the standard cell potential.
In the given reaction, Zn(s) is oxidized to Zn$^{2+}$(aq) and Fe$^{2+}$(aq) is reduced to Fe(s).
Thus, n=2. E$^\circ$ = 0.32 V
\(\Delta G^\circ = -(2 mol)(96487 C mol^{-1})(0.32 V) \)
\(\Delta G^\circ = -61751.04 J mol^{-1} \approx -61.75 kJ mol^{-1}\)
The output (Y) of the given logic gate is similar to the output of an/a :
A | B | Y |
0 | 0 | 1 |
0 | 1 | 0 |
1 | 0 | 1 |
1 | 1 | 0 |
List I (Spectral Lines of Hydrogen for transitions from) | List II (Wavelength (nm)) | ||
A. | n2 = 3 to n1 = 2 | I. | 410.2 |
B. | n2 = 4 to n1 = 2 | II. | 434.1 |
C. | n2 = 5 to n1 = 2 | III. | 656.3 |
D. | n2 = 6 to n1 = 2 | IV. | 486.1 |