Question

Cd(s)+Cu+(aq)→Cd2+(aq)+Cu(s)

Answer 1

What's the question?

Answer 2

[AI-generated answer — Step-by-Step Bot]

The given chemical equation represents a redox reaction between solid cadmium (Cd) and aqueous copper ion (Cu+). Here are the step-by-step details of the reaction:

Step 1: Identify the oxidation state of each element before and after the reaction:
- Cd: It has an oxidation state of 0 before the reaction and +2 after the reaction.
- Cu: It has an oxidation state of +1 before the reaction and 0 after the reaction.

Step 2: Determine which element is being oxidized and which one is being reduced:
- Cd: It is being oxidized since its oxidation state increases from 0 to +2.
- Cu: It is being reduced since its oxidation state decreases from +1 to 0.

Step 3: Write the balanced half-reactions for oxidation and reduction:
Oxidation half-reaction: Cd(s) → Cd2+(aq) + 2e-
Reduction half-reaction: Cu+(aq) + e- → Cu(s)

Step 4: Balance the number of electrons transferred in the half-reactions by multiplying each half-reaction as necessary:
Oxidation half-reaction: Cd(s) → Cd2+(aq) + 2e-
Reduction half-reaction: 2Cu+(aq) + 2e- → 2Cu(s)

Step 5: Combine the half-reactions to form the final balanced equation:
Cd(s) + 2Cu+(aq) → Cd2+(aq) + 2Cu(s)

Thus, the balanced equation for the given reaction is Cd(s) + 2Cu+(aq) → Cd2+(aq) + 2Cu(s).

Answer 3

[AI-generated answer — Explain Bot]

The given chemical equation represents a redox (reduction-oxidation) reaction between solid cadmium (Cd) and aqueous copper ions (Cu+). In this reaction, cadmium is being oxidized and copper ions are being reduced.

To understand this reaction, we need to identify the oxidation states of each element involved:

Cd(s) → Cd2+(aq) (oxidation state of Cd changes from 0 to +2)
Cu+(aq) → Cu(s) (oxidation state of Cu changes from +1 to 0)

Now, let's break down the redox reaction step by step:

Step 1: Identify the half-reactions:
- Oxidation half-reaction: Cd(s) → Cd2+(aq)
- Reduction half-reaction: Cu+(aq) → Cu(s)

Step 2: Balance the atoms within each half-reaction:
- The number of cadmium (Cd) atoms on both sides of the equation is already balanced.
- The number of copper (Cu) atoms on both sides of the equation is already balanced.

Step 3: Balance the charges within each half-reaction:
- In the oxidation half-reaction, we have Cd(s) → Cd2+(aq) with a change in oxidation state from Cd(0) to Cd2+(+2). To balance the charges, we need to add two electrons (e-) to the left side of the equation: Cd(s) + 2e- → Cd2+(aq).
- In the reduction half-reaction, we have Cu+(aq) → Cu(s) with a change in oxidation state from Cu(+1) to Cu(0). To balance the charges, we don't need to add or subtract any electrons.

Step 4: Balance the number of electrons in both half-reactions:
- Since the number of electrons involved in the oxidation half-reaction (2e-) is equal to the number of electrons involved in the reduction half-reaction (2e-), we do not need to multiply either equation.

Step 5: Combine the half-reactions:
Now that both half-reactions are balanced, we can combine them to form the overall balanced reaction:

Cd(s) + 2Cu+(aq) → Cd2+(aq) + 2Cu(s)

In this reaction, solid cadmium (Cd) is oxidized to form aqueous cadmium ions (Cd2+), while copper ions (Cu+) are being reduced to form solid copper atoms (Cu).

I hope this explanation helps you understand the given redox reaction!