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Chlorine can be prepared by reacting HCl with MnO2. The reaction is represented by this...
Chlorine can be prepared by reacting HCl with MnO2. The reaction is represented by this equation.
MnO2(s) + 4HCl(aq) → Cl2(g) + MnCl2(aq) + 2H2O(l)
Assuming the reaction goes to completion what mass of concentrated HCl solution (36.0% HCl by mass) is needed to produce 2.50 g of Cl ?
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The balanced chemical equation for the reaction is:
`MnO_2(s) + 4HCl(aq)-> Cl_2(g) + MnCl_2(aq) + 2H_2O(l)`
So, `4*(35.5+1)=146 g` of `HCl` reacts with sufficient amount of `MnO_2` to produce `(35.5*2)=71 g` of chlorine.
In other words,
`71 g` of chlorine is obtained from `146 g` of `HCl` .
So, `2.50 g` of chlorine is obtained from `(146*2.50)/71=5.14 g` of `HCl`
In the conc. HCl solution,
`36 g` pure HCl is contained in `100 g HCl` solution.
So, `5.14 g HCl` is contained in `(100*5.14)/36=14.3 g HCl` solution.
Therefore, 14.3 g of conc. HCl solution is required to produce 2.50 g of chlorine.
Posted by llltkl on July 30, 2013 at 4:27 AM (Answer #1)
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