A gas occupies a volume of 2.4L at 740 torr pressure. What pressure will it occupy at 1.5atm?
Use P1V1 = P2V2
How do I cancel out the volume of Liters? Because it is asking for pressure.
A gas occupies a volume of 2.4L at 740 torr pressure. What pressure will it occupy at 1.5atm?
It appears to me that you have made a typo in posting the problem OR the question is flawed. I expect the question should be "what VOLUME will it occupy at 1.5 atm?
Assuming that is right, then
P1 = 740 torr = 740/760 = 0.974
V1 = 2.4 L
P2 = 1.5 atm
V2 = ?
So 0.974 atm x 2.4 L = 1.5 atm x V2
V2 = ?
If you answer the question as posted then the final pressure is 1.5 atm.
To solve this problem, we can use the combined gas law equation, which relates the initial and final pressures, volumes, and temperatures of a gas.
The combined gas law equation is stated as follows:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 and P2 are the initial and final pressures respectively,
V1 and V2 are the initial and final volumes respectively,
T1 and T2 are the initial and final temperatures respectively.
In this case, we have:
P1 = 740 torr
V1 = 2.4 L
P2 = ?
V2 = 2.4 L (since the volume remains constant)
T1 and T2 are not given, so we can assume they are constant.
Let's solve for P2 using the combined gas law equation:
(P1 * V1) / T1 = (P2 * V2) / T2
Since T1 and T2 are constant, we can simplify the equation to:
P1 * V1 = P2 * V2
Now plug in the given values:
(740 torr) * (2.4 L) = P2 * (2.4 L)
We can cancel out the common unit of volume (2.4 L):
740 torr = P2
Therefore, the gas will occupy a pressure of 740 torr at 1.5 atm.