Quote:
Originally Posted by jruiz3
Consider the following chemical equation.
2NO2 ----> N2O4
If 18.7 mL of NO2 gas is completely converted to N2O4 gas under the same conditions, what volume will the N2O4 occupy?
? mL
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I'm not a fan of this sort of question which says "under the same conditions". I think it's better to describe some actual conditions so that people think about the reality of the experiment.
When the number of moles of gas is halved, it's only possible to have "the same conditions" if the experiment is done in a flexible container, like a balloon. The volume will be halved in these circumstances.
BUT, if the reaction is carried out in a rigid container - most lab apparatus is rigid - the volume of the gas will stay the same. (A gas will always spread out to fully occupy a container.) Then, instead of the volume being halved, the pressure will be halved.