Answer:
1st answer choice
P4O6 + 2 O2 -> P4O10
Explanation:
You need to cancel out reactants and products that are the same.
P4 cancels out because it appears in both reactants and products
We get 2 O2 in the reactants because 5-3= 2
Thus, answer choice 1 is correct.
I believe C is the answer forgive me if i'm wrong
Explanation:
We know that,
= -0.7618 V
= 0.337 V
According to the given reaction/cell notation, cathode is (
and anode is ().
Therefore, 
= (0.337) - (-0.7618)
= 1.0988 V
In the given reaction, number of electrons being transferred in balanced reaction are 2. Hence, n = 2.
Also, we know that
E = ![E^{o} - (\frac{2.303 \times RT}{nF}) log {\frac{[Zn^{2+}]}^{1}{[Cu^{2+}]^{1}}](https://tex.z-dn.net/?f=E%5E%7Bo%7D%20-%20%28%5Cfrac%7B2.303%20%5Ctimes%20RT%7D%7BnF%7D%29%20log%20%7B%5Cfrac%7B%5BZn%5E%7B2%2B%7D%5D%7D%5E%7B1%7D%7B%5BCu%5E%7B2%2B%7D%5D%5E%7B1%7D%7D)
Putting the given values into the above formula as follows.
E = ![E^{o} - (\frac{2.303 \times RT}{nF}) log {\frac{[Zn^{2+}]}^{1}{[Cu^{2+}]}^{1}](https://tex.z-dn.net/?f=E%5E%7Bo%7D%20-%20%28%5Cfrac%7B2.303%20%5Ctimes%20RT%7D%7BnF%7D%29%20log%20%7B%5Cfrac%7B%5BZn%5E%7B2%2B%7D%5D%7D%5E%7B1%7D%7B%5BCu%5E%7B2%2B%7D%5D%7D%5E%7B1%7D)
=
=
= 1.0704 V
= 1.07 V (approx)
Thus, we can conclude that the cell voltage under these conditions is 1.07 V.