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brilliants [131]
3 years ago
14

A 20.7167 g sample of impure magnesium carbonate was heated to complete decomposition according to the equation mgco3(s) → mgo(s

) + co2(g). after the reaction was complete, the solid residue (consisting of mgo and the original impurities) had a mass of 16.8817 g. assuming that only the magnesium carbonate had decomposed, how much magnesium carbonate was present in the original sample? answer in units of g. 013 5.0 points the reaction of 8.9 grams of fluo
Chemistry
1 answer:
marishachu [46]3 years ago
5 0

The mass of impure MgCO_{3} is 20.7167 g. The decomposition reaction is as follows:

MgCO_{3}(s)\rightarrow MgO(s)+CO_{2}(g)

Here, 1 mole of MgCO_{3} gives 1 mole of MgO.

Molar mass of MgCO_{3}  and MgO is 84.31 g/mol and 40.3044 g/mol respectively.

Converting number of moles in terms of mass,

n=\frac{m}{M}

Here, M is molar mass.

Since, n_{MgCO_{3}}=n_{MgO}

Thus, \frac{m_{MgCO_{3}}}{M_{MgCO_{3}}}=\frac{m_{MgO}}{M_{MgO}}

On putting the values,

\frac{m_{MgCO_{3}}}{84.31}=\frac{m_{MgO}}{40.3044}

Rearranging,

m_{MgO}=\frac{m_{MgCO_{3}}}{84.31}\times 40.3044

Or,

m_{MgCO_{3}}=\frac{m_{MgO}}{0.4780}...... (1)

Let the mass of impurity be M_{I}  and mass of impure MgCO_{3} is 20.7167 g thus,

M_{MgCO_{3}}=(20.7167-M_{I})g...... (2)

Also, mass of impure MgO is 16.8817 g thus,

M_{MgO}=(16.8817-M_{I})g...... (3)

On comparing equations (2) and (3),

M_{MgO}=M_{MgCO_{3}}-3.835

Putting the value of M_{MgO} in equation (1),

m_{MgCO_{3}}=\frac{M_{MgCO_{3}}-3.835}{0.4780}

Or,

0.4780 M_{MgCO_{3}}=M_{MgCO_{3}}-3.835

Or,

M_{MgCO_{3}}-0.4780M_{MgCO_{3}}=3.835

Or,

0.522 M_{MgCO_{3}}=3.835

Or,

M_{MgCO_{3}}=\frac{3.835}{0.522}=7.35 g

Thus, magnesium carbonate present in the original sample is 7.35 g.


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