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Chapter 4: 4.6 CYL (page 191)

This equation describes the production of tin (II) chloride.\(Sn\left( s \right) + 2HCl\left( g \right) \to SnC{l_2}\left( s \right) + {H_2}\left( g \right)\)Is this a redox reaction? If so, provide a more specific name to the reaction if appropriate, and identify the oxidant and reductant.

Short Answer

Expert verified

Yes, it is a redox reaction, and a single replacement reaction. Sn(s) is the reductant and HCl(g) is the oxidant in the given reaction.

Step by step solution

01

Redox reaction

The given reaction is a redox reaction as the oxidation number of one element increases while the other decreases (i.e., one element oxidizes and the other reduces). Here, Sn goes from 0 to 2 while H goes from 1 to 0.

02

Oxidant and reductant

\(2H\left( I \right) + 2e \to 2H\left( 0 \right):\)Here, the oxidation number in H goes from 1 to 0, hence reduction occurs.

\(Sn\left( 0 \right) - 2e \to Sn\left( {II} \right):\) Here, the oxidation state in Sn goes from 0 to 2, hence oxidation occurs.

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Most popular questions from this chapter

Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60掳C), filtering to remove insoluble impurities, cooling to 0 掳C to precipitate solid NaHCO3 , and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 掳C is 164 g/L. Its solubility in cold water of 0 掳C is 69 g/L. What is the percent yield of NaHCO3 when it is purified by this method?

Diatomic chlorine and sodium hydroxide(lye) are commodity chemicals produced in large quantities, along with diatomic hydrogen via the electrolysis of brine according to the following unbalanced equation:

\[NaCl\left( {aq} \right) + {H_2}O\left( l \right) \to NaOH\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right).\]

Write balanced molecular, complete ionic, and net ionic equations for this process.

Complete and balance each of the following oxidation-reduction reactions,such that it results in the highest possible oxidation state for the oxidized atoms.

(a) \(Al\left( s \right) + {F_2}\left( g \right) \to \)

(b) \(Al\left( s \right) + CuB{r_2}\left( {aq} \right) \to \) (single displacement)

(c) \({P_4}\left( s \right) + {O_2}\left( g \right) \to \)

(d) \(Ca\left( s \right) + {H_2}O\left( l \right) \to \) (products are a strong base and a diatomic gas)

How many moles of Ca(OH)2 are required to react with 1.36 mol of H3PO4 to produce Ca3(PO4)2 according to the equation \(3Ca{\left( {OH} \right)_2} + 2{H_3}P{O_4} \to C{a_3}{\left( {P{O_4}} \right)_2} + 6{H_2}O\)?

Write a balanced molecular equation describing each of the following chemical reactions.

(a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas

(b)Gaseous butane reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor

(c)Aqueous solution of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride

(d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.
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