Magnesium reacts with titanium(4) chloride to produce magnesium chloride and titanium metal. How do you write a balanced equation for this reaction?

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Magnesium reacts with titanium(4) chloride to produce magnesium chloride and titanium metal. How do you write a balanced equation for this reaction?

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Answer 1 · 2016-12-18T11:21:29

$2 M g + T i C l_{4} \to 2 M g C l_{2} + T i$ $2 Mg + TiCl_4 rarr 2 MgCl_2 + Ti$

Explanation:

Because the magnesium ion has a +2 charge, the formula for magnesium chloride is $M g C l_{2}$ $MgCl_2$ .

To balance the four Cl ions in titanium (IV) chloride, the reaction must produce 2 units of $M g C l_{2}$ $MgCl_2$

Answer 2 · 2016-12-18T11:22:42

$T i C l_{4} + 2 M g \to T i + 2 M g C l_{2}$ $TiCl_4 + 2Mg rarr Ti + 2MgCl_2$

Explanation:

We could do this by individual redox steps:

$T i C l_{4} + 4 e^{-} \to T i + 4 C l^{-}$ $TiCl_4 + 4e^(-) rarr Ti + 4Cl^-$ $(i)$ $(i)$

$M g \to M g^{2 +} + 2 e^{-}$ $Mgrarr Mg^(2+) + 2e^-$ $(i i)$ $(ii)$

$(i) + 2 \times (i i) =$ $(i) + 2xx(ii)=$ $T i C l_{4} + 2 M g \to T i + 2 M g C l_{2}$ $TiCl_4 +2Mgrarr Ti +2MgCl_2$

With all chemical reactions, 2 conditions must be absolutely satisfied: (i) mass must be balanced; and (ii) charge must be balanced. Well, is they?

Note that just because I can write the reaction, there is no likelihood that the reaction can be performed. Should I attempt to reduce the chloride with magnesium metal I would likely get a mess. Titanic chloride is unstable with respect to water and dioxygen.

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Magnesium reacts with titanium(4) chloride to produce magnesium chloride and titanium metal. How do you write a balanced equation for this reaction?

2 Answers

Explanation:

Explanation:

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