Answer:
Option C. Cu is oxidized at the anode and Ag+ is reduced at the cathode.
Explanation:
The reaction that is taking place in the voltaic cell is:
Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)
A voltaic cell is an electrochemical cell that uses spontaneous redox reactions, like the above, to generate electricity.
In the rection above, the electrode of the anode is Cu, and the electrode of the cathode is Ag. In the cell, the solution of Ag⁺ produces the oxidation of the Cu(s) which results in Cu²⁺ and Ag(s) (since the Ag⁺ is being reduced). In a voltaic cell, the anode is the electrode at which the oxidation reaction occurs and the cathode is the electrode at which the reduction reaction takes place.
The redox reactions in this system release energy, so a wire connects the two reactions and allows electrons to flow from one side to the other, forming the Voltaic (or Galvanic) Cell.
From all of the above, the correct option is c: Cu is oxidized at the anode, and Ag+ is reduced at the cathode.
I hope it helps you!
Energy and oreantation its one if not bolth of those
The balanced complete ionic equation for HI(aq) + RbOH(aq) →RbI(aq) +H2O(l) is given by;
Net ionic equation; H+(aq) + OH-(aq) → H2O(l)
<h2>Further Explanation:
</h2><h3>Balancing chemical equation:
</h3>
- Balancing chemical equations is a try and error method that ensures the number of atoms in the side of the reactants is equal to the number of atoms in the side of products.
- Balancing chemical equations ensures that the law of conservation of mass is observed.
- Balancing chemical equations may also require inclusion of state symbols which shows the state of each compound or element involved in the chemical reaction.
<h3>Net ionic equations </h3>
- Net ionic equations that do not include all ions that are present in the reactants and products.
- The equations only includes the ions that are involved in the reaction.
- The ions that are not involved in a chemical reaction are called spectator ions and are cancelled out while writing ionic equations.
A reaction between HI and RbOH is given by;
HI(aq) + RbOH(aq) →RbI(aq) + H2O(l)
- The ionic equation for the reaction will be;
H+(aq) + I-(aq) + Rb+(aq) + OH-(aq) → H2O(l) + Rb+(aq) + I-(aq)
- H+ changes state from aqueous to liquid, OH- changes state from aqueous to liquid, while both Rb+ and I- do not change state and thus are not included while writing the net ionic equation.
Therefore;
Net ionic equation will be;
H+(aq) + OH-(aq) → H2O(l)
Keywords: Net ionic equations
<h3>Learn more about; </h3>
Level: High school
Subject: Chemistry
Topic: Chemical equation
Sub-topic: Net ionic equations
<u>Answer:</u> The correct answer is Option B.
<u>Explanation:</u>
Oxidizing agent is the agent which oxidizes the other substance and itself gets reduced. It undergoes reduction reaction in which, it gains electrons and also the oxidation state of the substance gets reduced.
Reducing agent is the agent which reduces the other substance and itself gets oxidized. It undergoes oxidation reaction in which, it looses electrons and the oxidation state of the substance is increased.
For the given chemical equation:
![Cu+2AgNO_3\rightarrow 2Ag+Cu(NO_3)_2](https://tex.z-dn.net/?f=Cu%2B2AgNO_3%5Crightarrow%202Ag%2BCu%28NO_3%29_2)
Half reactions for the given chemical reaction:
![Cu\rightarrow Cu^{2+}+2e^-](https://tex.z-dn.net/?f=Cu%5Crightarrow%20Cu%5E%7B2%2B%7D%2B2e%5E-)
Copper is loosing 2 electrons, thus it is undergoing oxidation reaction and is considered as a reducing agent.
![Ag^++e^-\rightarrow Ag](https://tex.z-dn.net/?f=Ag%5E%2B%2Be%5E-%5Crightarrow%20Ag)
Silver ion is gaining 1 electron per atom, thus it is undergoing reduction reaction and is considered as an oxidizing agent.
Hence,
is considered as an oxidizing agent and therefore the correct answer is Option B.