A gas has pressure of 4.62 atm when its volume is 2.33 L if the temperature remains constant, what will the pressure be when the volume is changed to 1.03 L? express the final pressure in torrs
Try the P1V1/T1 = P2V2/T2 thing I showed you last night. I shall be happy to check you answer.
To solve this problem, we can use the combined gas law equation:
(P1 * V1) / T1 = (P2 * V2) / T2
Given:
P1 = 4.62 atm
V1 = 2.33 L
V2 = 1.03 L
T1 and T2 remain constant
Now, let's rearrange the equation to solve for P2:
P2 = (P1 * V1 * T2) / (V2 * T1)
Substituting the given values:
P2 = (4.62 atm * 2.33 L * T2) / (1.03 L * T1)
Since the temperature remains constant, we can omit it:
P2 = (4.62 atm * 2.33 L) / 1.03 L
P2 = 10.73 atm
Now, to express the final pressure in torr, we can use the conversion factor:
1 atm = 760 torr
P2_torr = P2 * 760 torr
P2_torr = 10.73 atm * 760 torr
P2_torr = 8148.8 torr
Therefore, the final pressure will be approximately 8148.8 torr when the volume is changed to 1.03 L.