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Elan Coil [88]
3 years ago
11

Gaseous BF3 and BCl3 are mixed in equal molar amounts. All B-F bonds have about the same bond enthalpy, as do all B-Cl bonds. Co

mpare the numbers of microstates to explain why the mixture tends to react to form BF2Cl(g) and BCl2F(g
Chemistry
1 answer:
lord [1]3 years ago
8 0

Solution :

$BF_3 (g) + BCl_3 (g) \rightarrow BF_2 Cl + BCl_F(g)$

<u>Explanation 1 </u>:

Spontaneity of the reaction is based on two factors :

-- the tendency to acquire a state of minimum energy

-- the energy of a system to acquire a maximum randomness.

Now, since there isn't much difference in the bond enthalpies of B-F and B-Cl. So, we can say the major driving factor is tendency to acquire a state of maximum randomness.

<u>Explanation 2 </u>:

A system containing the \text{"chemically mixed"} B halides has a \text{greater entropy} than a system of $BCl_3$ and BF_3.

It has the same number of \text{gas phase molecules}, but more distinguishable kinds of \text{molecules}, hence, more microstates and higher entropy.

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