500 mL Of hydrogen at 27 degrees celcius and 3 atms pressure is compressed to 100 mL at 100 degrees celsius. What is the new pressure in atms?
To calculate the new pressure in atmospheres (atm), we can use the combined gas law equation, which relates the initial and final states of a gas:
(P1 ⨉ V1) / (T1 - 273) = (P2 ⨉ V2) / (T2 - 273)
Where:
P1 = initial pressure (in atm)
V1 = initial volume (in mL)
T1 = initial temperature (in Celsius)
P2 = final pressure (in atm)
V2 = final volume (in mL)
T2 = final temperature (in Celsius)
Let's plug in the given values into the equation:
(P1 ⨉ 500) / (27 - 273) = (P2 ⨉ 100) / (100 - 273)
Next, let's convert the temperatures from Celsius to Kelvin by adding 273 to each:
(P1 ⨉ 500) / (27 + 273) = (P2 ⨉ 100) / (100 + 273)
Simplifying the equation further:
500P1 / 300 = 100P2 / 373
Now, let's rearrange the equation to solve for P2:
P2 = (500P1 ⨉ 373) / (100 ⨉ 300)
Let's substitute in the value of P1, which is 3 atm:
P2 = (500 ⨉ 3 ⨉ 373) / (100 ⨉ 300)
Simplifying the equation:
P2 = 55950 / 30000
P2 ≈ 1.865 atm
Therefore, the new pressure in atmospheres is approximately 1.865 atm.
(P1V1/T1) = (P2V2/T2)
Remember T must be in kelvin. You spelled celsius wrong in this post but right in the previous post.