Question

A chemist places 1.72 mil of O2(g) and 2.88 mil of H2(g) into a rigid and sealed 7.50 L container.

a) calculate the total pressure in the container at 405 K
b) at low temperatures, the total pressure in the container is less than the value predicted using the Ideal Gas Law. Explain this phenomenon
c) a lab technician ignites the mixture in the container and the following reaction occurs: 2H2(g) + O2(g) —> 2H2O(g). Find the partial pressure of 02(g) in the container at 405 K after the reaction has gone to completion.

Answer 1

I'm confused. Does mil your abbreviation for mol or mL. And if it is mL what are the conditions at which the volume was measure; i.e., If you are place 1.72 mL O2 INTO a sealed container then we need to know the volume before those gases were introduced into the container. Please clarify.