A gas occupies 56.44 L at 2.00 atm and 310 K. If the gas is compressed to 23,520 mL and the temperature is lowered to 281 K, what is the new pressure in torr?
(P1V1/T1) = (P2V2/T2)
Make sure V1 and V2 are in the same units. I would change 2 atm and use P1 as 760 x 2 = ? torr. That way the asnwer will come out in torr.
To find the new pressure in torr, we can use the combined gas law equation:
(P1 * V1) / (T1) = (P2 * V2) / (T2)
Where:
P1 = initial pressure in atm
V1 = initial volume in liters
T1 = initial temperature in Kelvin
P2 = final pressure (what we want to find) in atm
V2 = final volume in liters
T2 = final temperature in Kelvin
Given:
P1 = 2.00 atm
V1 = 56.44 L
T1 = 310 K
V2 = 23,520 mL = 23.52 L
T2 = 281 K
Now, let's plug in the given values into the combined gas law equation and solve for P2:
(2.00 atm * 56.44 L) / 310 K = (P2 * 23.52 L) / 281 K
First, let's simplify the left side of the equation:
(112.88 atm * L) / K = (P2 * 23.52 L) / 281 K
Next, cross-multiply and solve for P2:
112.88 * 281 = P2 * 23.52
31,739.28 = P2 * 23.52
Now, divide both sides of the equation by 23.52 to isolate P2:
P2 = 31,739.28 / 23.52
P2 ≈ 1,348.49
Therefore, the new pressure in torr is approximately 1,348.49 torr.