Non metal i believe let me know if i helped
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where, E^{o} (Ag+/Ag) = std. reduction potential of Ag+ = 0.7994 v
and Sn2+/Sn = std. reduction potential of Sn2+ = -0.14 v
Thus, E^{o}cell = 0.7994v - (-0.14v) = 0.9394 v
Now, ΔG^{o} = -nF
,
where, n = number of electrons = 2
F = Faraday's constant = 96500 C
∴ΔG^{o} = 2 X 96500 X 0.9394 = -1.18 X
Now, using Nernst's Equation we have,
![[tex]E_{cell} = 0.9394 - \frac{2.303X298}{2X96500}log \frac{0.0115}{ 3.5^{2} }](https://tex.z-dn.net/?f=%20%5Btex%5DE_%7Bcell%7D%20%3D%200.9394%20-%20%5Cfrac%7B2.303X298%7D%7B2X96500%7Dlog%20%5Cfrac%7B0.0115%7D%7B%203.5%5E%7B2%7D%20%7D%20)
E_{cell} = 0.9765 v
Finally, ΔG = -nFE = -2 X 96500 X 0.9765 = -1.88 X
A. 2 is the answer let me know if im wrong sorry if i am.
THE COMPLETE QUESTION IS:
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid . a. NH+4 b. Na+ c. Co3+ d. CH2NH+3
Answer:
<em>a. Acidic</em>
<em>b. neutral</em>
<em>c. Acidic</em>
<em>d. Acidic</em>
Explanation:
a. NH4+ + H2O <==> NH3 + H3O+ (NH4+ is a conjugate acid of a weak base. Therefore it is acidic)
b. Neutral. Na+ is a cation of a strong base. Therefore it's pH is neutral.
c. Co(H2O)6³+ + H2O <==>CoH2O5(OH)²+ + H3O+
(Therefore Co+ is a weak acid since hydronium ion is formed.)
d. CH2NH3+ is a conjugate acid of a weak base. Therefore it is acidic.
The answer to your question is the option D, it moves crust plates around
