Redox Reactions

Which of the following is an example of an oxidizing agent?

Removal of oxygen from a compound is called:

In the reaction $Mg + 2Ag^{+} \rightarrow Mg^{2+} + 2Ag$, the species being oxidized is:

The oxidation number of Oxygen in superoxides like $KO_{2}$ is:

In the redox reaction between copper and dilute nitric acid: $3Cu + 8HNO_{3} \rightarrow 3Cu(NO_{3})_{2} + 2NO + 4H_{2}O$, the following diagram represents the transformation of the central elements. Based on the electronic concept of redox reactions, what is the change in the oxidation state of the element that acts as the oxidizing agent?

In the balanced equation $aMnO_{4}^{-} + bC_{2}O_{4}^{2-} + cH^{+} \rightarrow dMn^{2+} + eCO_{2} + fH_{2}O$, what is the ratio of $a$ to $b$?

What is the oxidation state of Boron in $NaBH_{4}$?

When Ammonium dichromate $(NH_{4})_{2}Cr_{2}O_{7}$ is heated, it decomposes into Nitrogen gas, Chromium(III) oxide, and Water. Which of the following describes the redox change in Nitrogen and Chromium?

What is the oxidation state of Sulfur in Sulfur dichloride ($SCl_{2}$)?

In Chlorine dioxide ($ClO_{2}$), an unusual paramagnetic molecule, the oxidation state of Chlorine is:

If a substance 'X' can easily lose electrons to substance 'Y', then 'X' is a stronger _______ than 'Y'.

In the redox reaction $Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu$, which substance is the electron acceptor?

What is the role of chlorine in the reaction $2Na + Cl_2 \rightarrow 2NaCl$?

During the reduction of $Fe^{3+}$ to $Fe^{2+}$, the species:

A metal rod $X$ is dipped into a solution containing $Y^{2+}$ ions. If no reaction occurs, what can we conclude about the electron-donating ability of $X$ compared to $Y$?

In the reaction $2H_2S + SO_2 \rightarrow 3S + 2H_2O$, which species is losing electrons?

Identify the oxidizing agent in the following reaction: $Pb(s) + PbO_2(s) + 2H_2SO_4(aq) \rightarrow 2PbSO_4(s) + 2H_2O(l)$

In the process of electrolysis of molten $NaCl$, at the cathode, sodium ions ($Na^+$) are converted to sodium metal ($Na$). This process is an example of:

In the reaction $K_2Cr_2O_7 + 4H_2SO_4 + 3H_2S \rightarrow K_2SO_4 + Cr_2(SO_4)_3 + 7H_2O + 3S$, which statement is true about the electron transfer?

If a metal $M$ forms a cation $M^{n+}$ by losing $n$ electrons, and $0.1$ mole of $M$ releases $0.3$ moles of electrons, what is the formula of the oxide of this metal?

In Potassium Sulfide ($K_{2}S$), what is the oxidation number of Potassium?

In Nitrous Oxide ($N_{2}O$), what is the oxidation state of Nitrogen?

What is the oxidation state of Carbon in Carbon Dioxide ($CO_{2}$)?

According to the IUPAC rules, what is the sum of the oxidation numbers of all atoms in the Phosphate ion ($PO_{4}^{3-}$)?

What is the oxidation state of Uranium ($U$) in the Uranyl ion ($UO_{2}^{2+}$)?

In Ammonium Nitrate ($NH_{4}NO_{3}$), what are the oxidation states of the two Nitrogen atoms respectively?

Identify the oxidation state of Antimony ($Sb$) in the $SbF_{6}^{-}$ ion.

Allene ($C_{3}H_{4}$) has a structure where a central carbon atom is connected to two terminal carbon atoms through double bonds. By considering the structural arrangement and the relative electronegativity values of the atoms, what are the individual oxidation states of the terminal carbon atoms (C1 and C3) and the central carbon atom (C2) respectively?

In the complex ion $[Co(NH_{3})_{5}Cl]^{2+}$, what is the oxidation state of the Cobalt atom?

Determine the oxidation state of Nitrogen in the molecule $N_{2}O$ (Nitrous oxide).

In the balanced equation $H_2S + HNO_3 \rightarrow S + NO + H_2O$, what is the ratio of coefficients of $H_2S$ to $HNO_3$?

If you are balancing a reaction and you find that the number of electrons lost is 2 and gained is 3, by what factors should you multiply the half-reactions to equalize electrons?

What is the oxidation number of $Cr$ in $K_2CrO_4$?

Which ion is used to balance the charge in a basic medium during the half-reaction method?

When balancing $As_2S_3 + HNO_3 + H_2O \rightarrow H_3AsO_4 + H_2SO_4 + NO$, what is the coefficient of $NO$?

In balancing the reaction $H_2O_2 + PbS \rightarrow PbSO_4 + H_2O$, how many moles of $H_2O_2$ are consumed per mole of $PbS$?

What is the coefficient of $H^+$ when the following is balanced: $MnO_4^- + SO_2 + H_2O \rightarrow Mn^{2+} + HSO_4^- + H^+$?

When balancing the reaction $K_4[Fe(CN)_6] + KMnO_4 + H_2SO_4 \rightarrow Fe_2(SO_4)_3 + CO_2 + HNO_3 + MnSO_4 + K_2SO_4 + H_2O$, what is the total change in oxidation state (number of electrons lost) for one formula unit of $K_4[Fe(CN)_6]$?

In the reaction $Cr_2O_7^{2-} + I^- + H^+ \rightarrow Cr^{3+} + I_2 + H_2O$, what is the coefficient of $H^+$ in the balanced equation?

Oxidation of iodine by concentrated nitric acid yields iodic acid: $I_2 + HNO_3 \rightarrow HIO_3 + NO_2 + H_2O$. What is the coefficient of $H_2O$ in the balanced equation?

What happens to the oxidation number of an element during a reduction process?

Which of the following ions has an oxidation number of +1?

What is the oxidation number of Carbon in Glucose ($C_6H_{12}O_6$)?

In the electrochemical series, elements are arranged in increasing order of their:

Which of the following statements is correct regarding cell potential ($E_{cell}$)?

Consider the reaction $Ni(s) + 2Ag^+(aq) \rightarrow Ni^{2+}(aq) + 2Ag(s)$. The oxidation state of Nickel changes from:

In a $Cu-Ag$ galvanic cell ($E^\circ_{Cu^{2+}/Cu} = 0.34\ V$ and $E^\circ_{Ag^+/Ag} = 0.80\ V$), the silver electrode acts as the:

In the reaction $H_2S + HNO_3 \rightarrow NO + S + H_2O$, the ratio of coefficients for $H_2S$ and $HNO_3$ in the balanced equation is:

What is the oxidation number of Platinum in the complex ion $[PtCl_6]^{2-}$?

Which of the following is a redox reaction where the same element is both oxidized and reduced, but is NOT a disproportionation reaction (since the reactant starts with the element in two different oxidation states)?