Question

State the type of reactions each of the following equations represent

1. Cl2+2KBr→2KCl+Br2

2. 2MgO →2Mg+O2

3. PbO2 + SO2 →PbSO4

4. AgNO3+NaCl →AgCl+NaNO3​

Answer 1

Answer:

the answer is number 4 ok

Explanation:

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Answer 2

Answer:

Explanation:

Hey mate here is your answer:

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→1 : $Cl_{2}+2KBr$ ⇒ $2KCL+Br_2$.

→Answer: Reaction does not takes place as potassium is more reactive than chlorine.

If there is reaction it is displacement reaction. A+BC⇒AC+B.

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→2: $2MgO$ ⇒ $2Mg+O_2$.

→Answer : It is a combination reaction and an oxidation reaction where Mg is getting oxidized to form Mg O.

Hence it is a combination and oxidation reaction.

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→3: $PbO_2+SO_2$ ⇒ $PbSO_4$.

→Answer: Oxidation-reduction or redox reaction.

The type of reaction in which the substance involved in the reaction gains oxygen it is called an oxidation reaction.

On the other hand, the type of reaction in which the substance involved in the reaction loses oxygen it is called a reduction reaction.

The type of reaction in which out of two substances involved in the reaction, one loses the oxygen whereas the other gains the oxygen it is called redox or oxidation-reduction reaction.

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→$AgNO_3+NaCl$ ⇒ $AgCl+NaNo_3$.

→Answer: This reaction is an example of which type of reaction: NaCl + AgNO3 gives AgCl + NaNO3. Since there is an exchange of ions between the reactants, it is a double displacement reaction.

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Hope it helps you.