NEET Chemistry Questions: Redox Reactions & Electrochemisty

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How many mole ferrous $(Fe^{2+}) ion oxidized in ferric (Fe^{3+}) ion by the required no. of electrons the oretically to reduced 4 mole Cr_2O_7^{ 2– }in to Cr^{3+} $ ?




First, determine the total number of moles of electrons needed to reduce 4 moles of $Cr_2O_7^{2-}$ using the same half-reaction: $$4 imes 6 = 24 ext{ moles of electrons}$$. Since each $Fe^{2+}$ ion loses one electron to become $Fe^{3+}$, 24 moles of electrons will oxidize 24 moles of $Fe^{2+}$.
What mole of $MnO_4 ^– reduced in Mn^{2+} by the addition of 7.5 mole electrons in MnO_4 ^ –$ ?




No explanation available.
How many electrons required to add for the reduction of one mole of $MnO_4 ^ – in Mn^{2+} $ ?




No explanation available.
When $ 3.11 \times 10^{24} Cr_2O_7 ^{2–} ion reduced in Cr^{3+}, then how many ferrous (Fe^{2+}) ionoxidised in ferric (Fe^{3+}) $ ion ?




No explanation available.
Theoretically, how many moles of iodide $ (I^–) ion oxidized into iodate (IO_3 ^ –) in using the no of electrons required for the reduction of 24 moles of MnO_4 ^ – ion into Mn^{2+} $ ion ?




No explanation available.
What is the oxidation no. of underlined C in $ HCHO, CH_3CHO, CH_3COOCH_3 $ or formalehyde acetaldehyde, acetone respectively ?




No explanation available.
What is the oxidation no. of underlined C in $CH_3COOCH_3 $ respectively ?




No explanation available.
In which of the following compound, oxidation no of all C atoms are same ?




No explanation available.
What are the values of b, d and f in the balanced state of the following reaction? Reaction : $aMnO_4^ – +bAs_2 O_3^ + cH_2O \rightarrow dMn^{2+} + eASO_4 ^{ 3–} + fH ^+(P ^ H \lt 7) $




No explanation available.
In the balanced state of reaction, $aBr_2 + bOH ^– + CH_2O \rightarrow dBrO_4 ^ – + eHBr $ (basic medium), if c=9, then what will be the change in oxidation no. (change in no. of electrons).




No explanation available.
What will be the chage in the oxidation no. (change in no. of electrons) inbalanced eqation given below ? Reaction : $ 2S + bHNO_3 \rightarrow CH_2SO_4 + dNO $ (acidic medium)




No explanation available.
What will be the change in the oxidation no. (change in no. of electrons), if no. of $e^– = 10 in balanced eqation given below ? Reaction : aP_4 + bNO_3^ – + cH^+ \rightarrow dPO_4 3– + eNO_2 + fH_2O $ (acidic medium)




No explanation available.
What is the ratio of value of band c in the balanced equation given below ? Reaction: $ aP_4 + bNO_3 ^ – + CH^+ \rightarrow dPO_4 ^{3–} + eNO_2 + fH_2O (acidic medium)$




In the given reaction, we need to balance the chemical equation to find the ratio of the coefficients of $NO_3^-$ (b) and $H^+$ (c). After balancing the equation, it is found that the coefficients ratio b:c is 10:3. Hence, the correct answer is 10:3.
In the reaction, $ R – CHO + 2cuO \rightarrow R – COOH + Cu_2O $ which substance is oxidising agent? And which substance is oxidizes ? (mention it respectively)




In the given reaction, $R–CHO$ (an aldehyde) is oxidized to $R–COOH$ (a carboxylic acid), and $CuO$ (cupric oxide) is reduced to $Cu_2O$ (cuprous oxide). The oxidizing agent is the substance that gets reduced, which is $CuO$, and the substance that oxidizes is $R–CHO$. Thus, $CuO$ is the oxidizing agent, and $R–CHO$ is the substance being oxidized.
In which of the following reaction, $ H_2O_2 $ acts as oxidizing agent ?




No explanation available.