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

Question

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

Impact of this question

26997 views around the world

You can reuse this answer
Creative Commons License

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.

Science

Math

Humanities

... and beyond

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:

Related questions

Impact of this question