A sample of gas contains 0.1700 mol of HCl(g) and 8.500×10-2 mol of Br2(g) and occupies...
A sample of gas contains 0.1700 mol of HCl(g) and 8.500×10-2 mol of Br2(g) and occupies a volume of 14.2 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. L
Homework Answers
The reaction is carried out by consuming everything available from the reagents, since they were in stoichiometric amounts.
3 moles of gas are produced for every 3 moles of gas consumed, this means that the amount of moles is also a constant.
In conclusion we have that the final volume of the reaction is equal to the initial 14.2 L.
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