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A sample of gas contains 0.1500 mol of HCl(g) and 7.500×10-2 mol of Br2(g) and occupies a volume of 9.63 L. The following reaction takes place: 2HCl(g) + Br2(g)2HBr(g) + Cl2(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

Respuesta :

sebassandin

Answer:

9.63 L.

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

[tex]2HCl(g) + Br_2(g)\rightarrow 2HBr(g) + Cl_2(g)[/tex]

So the consumed amounts of hydrochloric acid and bromine are the same to the beginning based on:

[tex]n_{Br_2}^{consumed}=0.1500molHCl*\frac{1molBr_2}{2molHCl}=0.075molBr_2[/tex]

In such a way, the yielded moles of hydrobromic acid and chlorine are:

[tex]n_{HBr}=0.1500molHCl*\frac{2molHBr}{2molHCl}=0.1500molHBr \\n_{Cl_2}=0.1500molHCl*\frac{1molCl_2}{2molHCl}=0.075molCl_2[/tex]

Thus, the volume of the sample, after the reaction is the same as no change in the total moles is evidenced, that is 9.63L.

Best regards.

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