Answer:
a. -58 millivolts
Explanation:
The given Nernst equation is:
![E_{ion} = 58 millivolts /z \Big[ log_{10} \Big( \dfrac{[ion]_{out}}{[ion]_{in}}\Big) \Big]}](https://tex.z-dn.net/?f=E_%7Bion%7D%20%3D%2058%20millivolts%20%2Fz%20%5CBig%5B%20log_%7B10%7D%20%5CBig%28%20%5Cdfrac%7B%5Bion%5D_%7Bout%7D%7D%7B%5Bion%5D_%7Bin%7D%7D%5CBig%29%20%5CBig%5D%7D)
The equilibrium potential given by the Nernst equation can be determined by using the formula:
![E_{Cl^-} = \dfrac{2.303*R*T}{ZF} \times log \dfrac{[Cl^-]_{out}} {[Cl^-]_{in}}](https://tex.z-dn.net/?f=E_%7BCl%5E-%7D%20%3D%20%5Cdfrac%7B2.303%2AR%2AT%7D%7BZF%7D%20%5Ctimes%20log%20%5Cdfrac%7B%5BCl%5E-%5D_%7Bout%7D%7D%20%7B%5BCl%5E-%5D_%7Bin%7D%7D)
where:
gas constant(R) = 8.314 J/K/mol
Temperature (T) = (20+273)K
= 298K
Faraday constant F = 96485 C/mol
Number of electron on Cl = -1
3. Cl₂ + 2KI --> 2KCl + I₂
Cl = 2 Cl = 2
K = 2 K = 2
I = 2 I = 2
4. 2NaCl --> 2Na + Cl₂
Na = 2 Na = 2
Cl = 2 Cl = 2
5. 4Na + O₂ --> 2Na₂O
Na = 4 Na = 4
O = 2 O = 2
6. 2Na + 2HCl --> H₂ + 2NaCl
Na = 2 Na = 2
H = 2 H = 2
Cl = 2 Cl = 2
7. 2K + Cl₂ --> 2KCl
K = 2 K = 2
Cl = 2 Cl = 2
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