I am currently attempting the following problem:
Consider the flask diagrammed below. What are the final partial pressures of H2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3 L) What is the total pressure in torrs?
_________ _____________
l l l l
l 2L H2 l--------l----l---- --l 1L N2 l
l 475 torr l--------l----l-------l 0.2 atm l
l l l l
l________l l___________ l
Note: The thing in the middle is the stopcock
My attempt:
Dalton's Law states that the total pressure is the sum of the individual pressures of the gases as if they were in separate containers.
So the individual pressure of the 2 litres of H2 would be 475 torrs and the individual pressure of the 1 litre of N2 would be 0.2 atm (converting to torrs would be 0.2*760=152 torrs)
Hence the total pressure would be the sum of the two, so 475 + 152 = 604 torrs. And the partial pressures would be 475 torrs for H2 and 152 torrs for N2.
However, this differs from the actual answers. So what am I doing wrong?
Thank you in advance!