Two gases are contained in gas bulbs connected by a valve. Gas A is present in a 56 L bulb at a pressure of 213 torr. Gas B exerts a pressure of 683 torr in a 74 L bulb. What is the partial pressure of gas B after they
equilibrate once the valve has been opened? Answer in units of torr.
How many moles are in gas A?
Use PV = nRT and solve for n.
How many moles are in gas B?
Solve for n for that gas.
Now, using PV = nRT and a NEW volume (the final volume = 74L+56L = ??L) calculate the P of each gas by itself.
There is a much easier way to do it.
P1V1 = P2V2 for each gas.
Thanks, I thought I could use Boyle's Law, but it seemed too easy.
0. 632atm
To find the partial pressure of gas B after the valve has been opened and both gases have equilibrated, we can use Dalton's law of partial pressures. According to Dalton's law, the total pressure exerted by a mixture of non-reacting gases is the sum of the partial pressures of each individual gas.
First, let's calculate the partial pressure of gas A. Gas A is in a 56 L bulb at a pressure of 213 torr. Therefore, the partial pressure of gas A is 213 torr.
Next, let's calculate the partial pressure of gas B. Gas B is in a 74 L bulb at a pressure of 683 torr. Therefore, the partial pressure of gas B is 683 torr.
Now, we can use Dalton's law to determine the total pressure exerted by the mixture of gases after equilibration.
Total pressure = Partial pressure of gas A + Partial pressure of gas B
Total pressure = 213 torr + 683 torr
Total pressure = 896 torr
Therefore, the partial pressure of gas B after equilibration is 896 torr.