Redox Reaction

Q. What do you observe? When​

(d) $H_{2}S$ gas is passed through copper sulphate solution.

Q. Name​
(a) a carbonate which does not decompose on heating.​

Q.

Potassium (at No. 19) and chlorine (at No. 17) form a compound. Explain the formation of the compound on the basis of :

(a) oxidation (b) reduction

(c) oxidising agent (d) reducing agent.

Q.

Hydrogen peroxide oxidises [Fe(CN)₆]^4- to [Fe(CN)₆]^3- in acidic medium but reduces [Fe(CN)₆]^3- to [Fe(CN)₆]^4- in alkaline medium. The other products formed are, respectively.

1. (H₂O+O₂) and (H₂O+OH^–)

2. H₂O and (H₂O+O₂)

3. H₂O and (H₂O+ OH^–)

4. (H₂O+O₂) and H₂O

Q.

Divide the following redox reactions into oxidation and reduction half reactions.

(i) $Zn+P{b}^2\to Z{n}^2+Pb$

(ii) $Zn+C{u}^{2+}\to Z{n}^2+Cu$

(iii) $C{l}_2+2B{r}^{-}\to B{r}_2+2C{l}^{-}$

Q.

Explain that the formation of magnesium chloride is a redox reaction.

Q.

A reducing agent is a substance which can donate electrons.

1. True

2. False

Q.

What do you understand by redox reactions ? Explain oxidation and reduction in terms of loss or gain of electrons.

Q.

Identify the following reactions as either oxidation or reduction :

(i) $O+2e^{-}\to O^{2-}$ (ii) $K-e^{-}\to K^{+}$ (iii) $F{e}^{3+}+e^{-}\to F{e}^{2+}$

Q.

State, giving reasons, whether the substances printed in bold letters have been oxidised or reduced.

(a) $PbO+CO\to Pb+C{O}_2$

(b) $H_{2}S+C{l}_2\to 2HCl+S$

Q.

How many electrons are lost by zinc during the process of oxidation?

1. 1

2. 2

3. 3

4. 4

Q. Loss of electrons in a chemical reaction is termed as ______.

1. oxidation
2. reduction
3. redox
4. electronegativity

Q.

State whether the following conversions are oxidation or reduction.

(a) $Pb{O}_2+S{O}_2\to PbS{O}_4$

(b) $K\to K^{+}{e}^{-}$

Q. Write a balanced chemical reaction and give your observation when the following metals react:​
Magnesium with steam​

Q.

Compare hydrogen with alkali metals on the basis of -

(i) Ion formation

(ii) Reducing power

(iii) Reaction with oxygen

(iv) Oxide formation

Q. State whether the following conversions are oxidation or reduction reactions.​
$Cu{}^2{}^{+}+2e^{-}\to Cu$

Q. Under what conditions can hydrogen be made to combine with: ​ Sulphur​
Name the product and write the reaction in each case.​

Q. Why is zinc and aluminum considered to have unique nature? Give balanced equations to support your answer.

Q. Copper oxide is heated with hydrogen to form copper metal & water. Identify the oxidising agent.

1. Copper
2. Copper oxide
3. Water
4. Hydrogen

Q.

Consider the diagram below to identify the gas X.

1. Oxygen
2. Water vapour
3. Hydrogen
4. Mixture of oxygen and hydrogen

Q. ${\text{CO}}_2\text{(g)}+{\text{H}}_2\text{(g)}\to \text{CO(g)}+{\text{H}}_2\text{O(l)}$

The given reaction is an example of:

1. decomposition reaction
2. redox reaction
3. combination reaction
4. precipitation reaction

Q. Assertion (A):​
Silver chloride is stored in dark-coloured bottles.​
Reason (R):​
Silver chloride undergoes thermal decomposition in the presence of light.

1. Both (A) and (R) are true but (R) is not the correct explanation for (A)​
2. Both (A) and (R) are true and (R) is the correct explanation for (A)​
3. Only (A) is true but (R) is false​
4. Both (A) and (R) are false​

Q. Silver reacts with hydrochloric acid to give $H_2$.

1. True
2. False

Q.

In reaction

$S{O}_2$ + $H_{2}S$ $\to$ $2H_{2}O$ + $3S$

the reducing agent is –

1. $S{O}_2$

2. $H_{2}S$

3. $H_{2}O$

4. $S$

Q. ${\text{CO}}_2\text{(g)}+{\text{H}}_2\text{(g)}\to \text{CO(g)}+{\text{H}}_2\text{O(l)}$

The given reaction is an example of:

1. combination reaction
2. precipitation reaction
3. decomposition reaction
4. redox reaction

Q. In which of the reactions, oxygen is an oxidant?

1. $2F_2+O_2\to 2F_{2}O$
2. $C+O_2\to C{O}_2$
3. $2C+O_2\to 2CO$
4. $2N_2+O_2\to 2N_{2}O$

Q. What do you understand by redox reaction? Explain oxidation and reduction in terms of loss or gain of electrons.

Q. <!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> Explain redox reactions based on electron transfer. Give suitable examples.

Q.

The reddish-brown fume coming out when lead nitrate is heated is known as

1. Nitrogen monoxide

2. Nitrogen

3. Nitrogen trioxide

4. Nitrogen dioxide