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  4. Redox Reactions Chapter-Wise Test 15

Redox Reactions Chapter-Wise Test 15

Correct answer Carries: 4.

Wrong Answer Carries: -1.

What is the oxidation number of bismuth in \( \ce{Bi2O3} \)?

Let Bi = \( x \). O = -2. Equation: \( 2x + 3(-2) = 0 \), \( 2x - 6 = 0 \), \( x = +3 \).

+5
+3
+2
+4
2

Which reaction involves a redox process where the reducing agent is a compound containing sulfur?

In \( \ce{SO2 + 2H2 -> S + 2H2O} \), \( \ce{SO2} \) (S: +4) is reduced to \( \ce{S} \) (0), oxidizing \( \ce{H2} \) (0 to +1).

\( \ce{2Na + Cl2 -> 2NaCl} \)
\( \ce{Fe + CuSO4 -> FeSO4 + Cu} \)
\( \ce{2H2O2 -> 2H2O + O2} \)
\( \ce{SO2 + 2H2 -> S + 2H2O} \)
4

In the reaction \( \ce{Sn + 2CuSO4 -> SnSO4 + Cu2SO4} \), what is the reducing agent?

The reducing agent loses electrons. Sn (0) oxidizes to \( \ce{Sn^2+} \) (+2), reducing \( \ce{Cu^2+} \) to \( \ce{Cu^+} \).

\( \ce{CuSO4} \)
\( \ce{Sn} \)
\( \ce{SnSO4} \)
\( \ce{Cu2SO4} \)
2

Which element is oxidized in the reaction \( \ce{2MnO2 + 4KOH + O2 -> 2K2MnO4 + 2H2O} \)?

Mn (+4 in \( \ce{MnO2} \)) increases to +6 in \( \ce{K2MnO4} \), losing electrons.

Oxygen
Potassium
Manganese
Hydrogen
3

In the reaction \( \ce{2NaI + Cl2 -> 2NaCl + I2} \), what is the reducing agent?

\( \ce{NaI} \) (I: -1 to 0 in \( \ce{I2} \)) loses electrons, reducing \( \ce{Cl2} \) (0 to -1).

\( \ce{Cl2} \)
\( \ce{NaCl} \)
\( \ce{I2} \)
\( \ce{NaI} \)
4

What is the change in oxidation number of nitrogen in the reaction \( \ce{N2 -> 2NH3} \) when balanced with H₂?

N (0 in \( \ce{N2} \)) becomes -3 in \( \ce{NH3} \). Change = -3 - 0 = -3.

+3
-3
+6
-6
2

In the reaction \( \ce{3Cu + 8HNO3 -> 3Cu(NO3)2 + 2NO + 4H2O} \), what is the oxidizing agent?

\( \ce{HNO3} \) (N: +5 to +2 in \( \ce{NO} \)) accepts electrons, oxidizing Cu (0 to +2).

\( \ce{Cu} \)
\( \ce{NO} \)
\( \ce{Cu(NO3)2} \)
\( \ce{HNO3} \)
4

For the reaction \( \ce{Sb2S3 + 6HCl -> 2SbCl3 + 3H2S} \), which species undergoes reduction?

Reduction is electron gain. Sb (+3 in \( \ce{Sb2S3} \)) remains +3 in \( \ce{SbCl3} \), but S (-2 to -2) doesn’t change; no reduction occurs here—it’s not redox.

None of these
\( \ce{Sb2S3} \)
\( \ce{HCl} \)
\( \ce{SbCl3} \)
1

Which of the following is a redox reaction involving a non-metal?

In \( \ce{P4 + 10Cl2 -> 4PCl5} \), P (0) is oxidized to +5, and Cl (0) is reduced to -1.

\( \ce{2Na + Cl2 -> 2NaCl} \)
\( \ce{CaO + CO2 -> CaCO3} \)
\( \ce{HCl + NH3 -> NH4Cl} \)
\( \ce{P4 + 10Cl2 -> 4PCl5} \)
4

Which reaction involves a redox process where the reducing agent contains phosphorus?

In \( \ce{P4 + 6Cl2 -> 4PCl3} \), \( \ce{P4} \) (P: 0 to +3) is oxidized, reducing \( \ce{Cl2} \) (0 to -1).

\( \ce{2Na + Cl2 -> 2NaCl} \)
\( \ce{P4 + 6Cl2 -> 4PCl3} \)
\( \ce{Fe + S -> FeS} \)
\( \ce{2H2O2 -> 2H2O + O2} \)
2

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