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Chapter 21: Problem 19

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) \(\mathrm{Br}_{2}(l)+\mathrm{I}^{-}(a q) \longrightarrow\)

Short Answer

Expert verified
(a) Cl2(g) + I⁻(aq) (b) F2(g) + Br⁻(aq) (c) I2(s) + Cl⁻(aq) (d) Br2(l) + I⁻(aq) Answer: (a) Yes, the reaction will occur. The balanced chemical equation is: Cl₂(g) + 2I⁻(aq) ⟶ 2Cl⁻(aq) + I₂(s) (b) Yes, the reaction will occur. The balanced chemical equation is: F₂(g) + 2Br⁻(aq) ⟶ 2F⁻(aq) + Br₂(l) (c) No, the reaction will not occur. (d) Yes, the reaction will occur. The balanced chemical equation is: Br₂(l) + 2I⁻(aq) ⟶ 2Br⁻(aq) + I₂(s)

Step by step solution

01

Use the activity series to determine possible reactions

For each of the given equations (a) to (d), we will use the activity series of halogens mentioned above to determine whether a halogen can replace another halogen in the compound.
02

(a) Determine the reaction for Cl2(g) + I⁻(aq)

Chlorine (Cl₂) is higher in the activity series than Iodine (I₂) and therefore can replace Iodine in the compound. So a reaction will occur.
03

(a) Complete and balance the reaction for Cl2(g) + I⁻(aq)

Cl₂(g) + 2I⁻(aq) ⟶ 2Cl⁻(aq) + I₂(s)
04

(b) Determine the reaction for F2(g) + Br⁻(aq)

Fluorine (F₂) is higher in the activity series than Bromine (Br₂) and therefore can replace Bromine in the compound. So a reaction will occur.
05

(b) Complete and balance the reaction for F2(g) + Br⁻(aq)

F₂(g) + 2Br⁻(aq) ⟶ 2F⁻(aq) + Br₂(l)
06

(c) Determine the reaction for I2(s) + Cl⁻(aq)

Iodine (I₂) is lower in the activity series than Chlorine (Cl₂) and therefore cannot replace Chlorine in the compound. So no reaction will occur.
07

(c) Write NR for no reaction

I₂(s) + Cl⁻(aq) ⟶ NR
08

(d) Determine the reaction for Br2(l) + I⁻(aq)

Bromine (Br₂) is higher in the activity series than Iodine (I₂) and therefore can replace Iodine in the compound. So a reaction will occur.
09

(d) Complete and balance the reaction for Br2(l) + I⁻(aq)

Br₂(l) + 2I⁻(aq) ⟶ 2Br⁻(aq) + I₂(s) The solutions for the given reactions are: (a) Cl₂(g) + 2I⁻(aq) ⟶ 2Cl⁻(aq) + I₂(s) (b) F₂(g) + 2Br⁻(aq) ⟶ 2F⁻(aq) + Br₂(l) (c) I₂(s) + Cl⁻(aq) ⟶ NR (d) Br₂(l) + 2I⁻(aq) ⟶ 2Br⁻(aq) + I₂(s)

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Most popular questions from this chapter

Chlorine can remove the foul smell of \(\mathrm{H}_{2} \mathrm{~S}\) in water. The reaction is $$\mathrm{H}_{2} \mathrm{~S}(a q)+\mathrm{Cl}_{2}(a q) \longrightarrow 2 \mathrm{H}^{+}(a q)+2 \mathrm{Cl}^{-}(a q)+\mathrm{S}(s)$$ If the contaminated water has \(5.0\) ppm hydrogen sulfide by mass, what volume of chlorine gas at STP is required to remove all the \(\mathrm{H}_{2} \mathrm{~S}\) from \(1.00 \times 10^{3}\) gallons of water \((d=1.00 \mathrm{~g} / \mathrm{mL}) ?\) What is the \(\mathrm{pH}\) of the solution after treatment with chlorine?

Give the formula for the acidic oxide of (a) \(\mathrm{HNO}_{3}\) (b) \(\mathrm{HNO}_{2}\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

Give the Lewis structure of (a) an oxide of nitrogen in the \(+5\) state. (b) the strongest oxoacid of nitrogen. (c) a tetrahedral oxoanion of sulfur.

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

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 \(\mathrm{SO}_{2} ?\)
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