Answer to Question #144945 in Chemistry for Lean Hangdaan

Question #144945
Chloroform, CHCl₃, is prepared industrially by the reaction of methane (CH₄) with chlorine. How many grams of Cl2 are needed to produce 1.50 moles of chloroform?
1
Expert's answer
2020-11-17T10:44:53-0500

The balanced equation for the reaction between methane and chlorine is:

CH4 + Cl2 "\\rightarrow" CH3Cl + HCl.

As it can be seen from this equation, when 1 mole of chlorine reacts, 1 mole of chloroform is formed:

"n(Cl_2) = n(CH_3Cl)" .

Therefore, to produce 1.50 moles of chloroform, the number of the moles of chloroform needed is also 1.50 moles.


The mass "m" of a compound can be calculated as a product of its number of the moles "n" and its molar mass "M" :

"m = n\\cdot M" .


The molar mass of chlorine is 70.91 g/mol. Thus, the mass of chlorine needed is:

"m(Cl_2) = 1.50\\text{ mol}\\cdot70.91\\text{ g\/mol} = 106.4" g.


Answer: 106.4 grams of Cl2 are needed to produce 1.50 moles of chloroform from methane.


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