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Chapter 20: Problem 17

At \(900^{\circ} \mathrm{C}\) titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction. (b) What is being oxidized, and what is being reduced? (c) Which substance is the reductant, and which is the oxidant?

Short Answer

Expert verified
a) The balanced equation for the reaction is \(TiCl_4 (g) + 2Mg (l) \rightarrow Ti (s) + 2MgCl_2 (l)\). b) Magnesium is being oxidized and titanium is being reduced. c) The reductant is molten magnesium (Mg) and the oxidant is titanium tetrachloride vapor (TiCl4).

Step by step solution

01

Write the reaction equation

To write the balanced equation, first write down the reactants and products: Reactants: Titanium tetrachloride vapor (TiCl4) and molten magnesium metal (Mg) Products: Solid titanium metal (Ti) and molten magnesium chloride (MgCl2) Now, we need to balance the equation: TiCl4 (g) + 2Mg (l) → Ti (s) + 2MgCl2 (l) The balanced equation is: \(TiCl_4 (g) + 2Mg (l) \rightarrow Ti (s) + 2MgCl_2 (l)\) ##Step 2: Identify the oxidation states of each element before and after the reaction##
02

Determine the oxidation states

We will determine the oxidation state of each element before and after the reaction: Before the reaction: - Ti in TiCl4: +4 - Cl in TiCl4: -1 - Mg: 0 After the reaction: - Ti: 0 - Cl in MgCl2: -1 - Mg in MgCl2: +2 ##Step 3: Determine which species is being oxidized and which is being reduced##
03

Identify oxidized and reduced species

In this reaction, the oxidation states of the elements change as follows: - Ti: +4 (TiCl4) → 0 (Ti), oxidation state decreases, so Ti is being reduced. - Mg: 0 (Mg) → +2(MgCl2), oxidation state increases, so Mg is being oxidized. ##Step 4: Identify the reductant and the oxidant##
04

Determine the reductant and the oxidant

The reductant is the species that reduces the other species by losing electrons. The oxidant is the species that oxidizes the other species by gaining electrons. In our reaction: - Mg (molten magnesium) is being oxidized, so it's the reductant. - TiCl4 (titanium tetrachloride vapor) is being reduced, so it's the oxidant. In conclusion: a) The balanced equation for the reaction is \(TiCl_4 (g) + 2Mg (l) \rightarrow Ti (s) + 2MgCl_2 (l)\). b) Magnesium is being oxidized and titanium is being reduced. c) The reductant is molten magnesium (Mg) and the oxidant is titanium tetrachloride vapor (TiCl4).

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Most popular questions from this chapter

(a) What is the maximum amount of work that a 6 -V lead-acid battery of a golf cart can accomplish if it is rated at \(300 \mathrm{~A}-\mathrm{h} ?(\mathrm{~b})\) List some of the reasons why this amount of work is never realized.

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