A #6 L# container holds #5 # mol and #6 # mol of gasses A and B, respectively. Groups of three of molecules of gas B bind to two molecules of gas A and the reaction changes the temperature from #480^oK# to #270^oK#. How much does the pressure change?
To calculate the initial pressure you can use the general law of perfect gasses: PV = nRT .
to know the final pressure, i suppose that there are still 3 moles of A, 3 moles of B and it was formed 1 mol of gas from the union of the moles reacted toward a total of 7 gass moles. The new pressure will be:
if instead all the molecules (6moles) of B react with the maximum possible number of the moles of A (4 moles, as the ratio is 3:2) at the end you will have still a mole of A and it was formed 2 moles of
I think that this second hypothesis is what is required