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Chapter 21: Problem 16

Write a balanced net ionic equation for (a) the oxidation of iodide to iodine by sulfate ion in acidic solution. Sulfur dioxide gas is also produced. (b) The preparation of iodine from an iodide salt and chlorine gas.

Short Answer

Expert verified
Answer: (a) 2 I^- + SO4^2- + 2 H^+ → I2 + SO2 + 2 H2O (b) 2 I^- + Cl2 → I2 + 2 Cl^-

Step by step solution

01

Write Unbalanced Equation

Write the unbalanced equation involving the reactants and products. 2 I^- + SO4^2- → I2 + SO2
02

Balance the atoms

The number of Iodine atoms is balanced. But for the Sulfur and Oxygen atoms, we can add water molecules (H2O) to balance the oxygen atoms and add hydrogen ions (H^+) to balance the hydrogen atoms. 2 I^- + SO4^2- + 2 H^+ → I2 + SO2 + 2 H2O
03

Write the balanced net ionic equation

Since no spectator ions are present in the reaction, the equation we obtained in the previous step is already a net ionic equation. The balanced net ionic equation is: 2 I^- + SO4^2- + 2 H^+ → I2 + SO2 + 2 H2O (b) Preparation of iodine from an iodide salt and chlorine gas
04

Write Unbalanced Equation

Write the unbalanced equation involving the reactants and products. The iodide salt reacts with chlorine gas (Cl2) to produce iodine (I2). 2 I^- + Cl2 → I2 + 2 Cl^-
05

Balance the atoms

All atoms (Iodine, Chlorine) are balanced in the equation, and there are no other atoms involved.
06

Write the balanced net ionic equation

Now, write the balanced net ionic equation. As there are no spectator ions in this reaction, the equation we have is the net ionic equation: 2 I^- + Cl2 → I2 + 2 Cl^-

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Most popular questions from this chapter

Why does concentrated nitric acid often have a yellow color even though pure \(\mathrm{HNO}_{3}\) is colorless?

Consider the reduction of nitrate ion in acidic solution to nitrogen oxide \(\left(E_{\mathrm{red}}^{\circ}=0.964 \mathrm{~V}\right)\) by sulfur dioxide that is oxidized to sulfate ion \(\left(E_{\text {red }}^{o}=0.155 \mathrm{~V}\right)\). Calculate the voltage of a cell involving this reaction in which all the gases have pressures of \(1.00 \mathrm{~atm}\), all the ionic species (except \(\left.\mathrm{H}^{+}\right)\) are at \(0.100 M\), and the \(\mathrm{pH}\) is \(4.30 .\)

Sulfur dioxide can be removed from the smokestack emissions of power plants by reacting it with hydrogen sulfide, producing sulfur and water. What volume of hydrogen sulfide at \(27^{\circ} \mathrm{C}\) and \(755 \mathrm{~mm} \mathrm{Hg}\) is required to remove the sulfur dioxide produced by a power plant that burns one metric ton of coal containing \(5.0 \%\) sulfur by mass? How many grams of sulfur are produced by the reaction of \(\mathrm{H}_{2} \mathrm{~S}\) with \(\mathrm{SO}_{2} ?\)

Complete and balance the following equations. If no reaction occurs, write NR. (a) \(\mathrm{Cl}_{2}(g)+\mathrm{Br}^{-}(a q) \longrightarrow\) (b) \(\mathrm{I}_{2}(s)+\mathrm{Cl}^{-}(a q) \longrightarrow\) (c) \(\mathrm{I}_{2}(s)+\mathrm{Br}^{-}(a q) \longrightarrow\) (d) \(\mathrm{Br}_{2}(l)+\mathrm{Cl}^{-}(a q) \longrightarrow\)

Complete and balance the following equations. If no reaction occurs, write NR. (a) \(\mathrm{Cl}_{2}(g)+\mathrm{I}^{-}(a q) \longrightarrow\) (b) \(\mathrm{F}_{2}(g)+\mathrm{Br}^{-}(a q) \longrightarrow\) (c) \(\mathrm{I}_{2}(s)+\mathrm{Cl}^{-}(a q) \longrightarrow\) (d) \(\mathrm{Br}_{2}(l)+\mathrm{I}^{-}(a q) \longrightarrow\)
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