Answer:
Yes because the law of conservation of matter is followed. There are equal numbers of atoms of all elements in the
reactants and products.
Explanation:
A balanced equation conform to the law of conservation of matter. While unbalanced equation suggests that matter has been created or destroyed.
Na3PO4 + 3KOH —> 3NaOH + K3PO4
A careful observation of the above equation proved that the equation is balanced is balanced because there are equal numbers of atoms of all elements in the
reactants and products.
The compounds that have covalent bonding as their dominant bonding scheme are diamond and silica.
A covalent bond is formed between two nonmetals. Usually, when two nonmetals combine, electrons are shared between the two atoms involved in the bond.
Now, the solids diamond and silica are predominantly covalent solids. The atoms that combine in diamond are carbon atoms(nonmetals) while the atoms that combine in silica are silicon and oxygen (nonmetals also)
Hence, diamond and silica both have covalent bonding as their dominant bonding scheme.
Learn more: brainly.com/question/11527546
We're given the [OH⁻] as 8.34 × 10⁻¹² M. Using the formula pOH = -log[OH⁻], the pOH of this solution would be -log(8.34 × 10⁻¹²) ≈ 11.08.
The pOH is, for lack of a better term, the "opposite" of pH: A pOH of 7 is neutral; a pOH less than 7 is <em>basic</em>; and a pOH greater than 7 is <em>acidic</em>.
This follows from the relation, pH + pOH = 14. In this case, with a pOH of 11.08, our pH would be 14 - 11.08 = 2.92, which is acidic (pH < 7).
Thus, the correct answer choice is B.
Answer: a) Anode: 
Cathode: 
b) Anode : Cr
Cathode : Au
c) 
d) 
Explanation: -
a) The element Cr with negative reduction potential will lose electrons undergo oxidation and thus act as anode.The element Au with positive reduction potential will gain electrons undergo reduction and thus acts as cathode.
At cathode:
At anode:
b) At cathode which is a positive terminal, reduction occurs which is gain of electrons.
At anode which is a negative terminal, oxidation occurs which is loss of electrons.
Gold acts as cathode ad Chromium acts as anode.
c) Overall balanced equation:
At cathode: (1)
At anode: (2)
Adding (1) and (2)
d)
= -0.74 V
= 1.40 V
Using Nernst equation :
![E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Au^{3+}]}{[Cr^{3+}]^}](https://tex.z-dn.net/?f=E_%7Bcell%7D%3DE%5Eo_%7Bcell%7D-%5Cfrac%7B0.0592%7D%7Bn%7D%5Clog%20%5Cfrac%7B%5BAu%5E%7B3%2B%7D%5D%7D%7B%5BCr%5E%7B3%2B%7D%5D%5E%7D)
where,
n = number of electrons in oxidation-reduction reaction = 3
= standard electrode potential = 2.14 V
![E_{cell}=2.14-\frac{0.0592}{3}\log \frac{[1.0}{[1.0]}](https://tex.z-dn.net/?f=E_%7Bcell%7D%3D2.14-%5Cfrac%7B0.0592%7D%7B3%7D%5Clog%20%5Cfrac%7B%5B1.0%7D%7B%5B1.0%5D%7D)
Thus the standard potential for an electrochemical cell with the cell reaction is 2.14 V.
