A scuba tank is filled to 2500 psi(170 atm) in a dive shop at room temp/(25 degrees C) then stored in the trunk of a car on a hot day. What will be the new pressure in the tank if the temp. in the trunk reaches 60 degrees C? Express that pressure in atmospheres, not psi.
(P1V1)/T1 = (P2V2)/T2
Use 170 atm for P1 and the answer will be in atm. Don't forget to use Kelvin for T1 and T2.
i don't understand this at alll
You plug in 170 atm for P1, there is no V1 or V2 in the problem, and T1 = 25 degrees C which si 273 + 25 = ??Kelvin. Continuing, P2 is what you want to know, V2 is not in the problem, and T2 is 60 degrees which must be convert to Kelvin. Then solve for P2.
okay so does it kinda look like this
(170)/298/333...i kinda understand not really
We have P1/T1 = P2/V2
You have P1 in the right place with the right number. Yuo have 298 ok. I don't see an equal sign. I don't see P2 (which you're solving for) and the 333 (the right number Kelvin) is not in the right place. Follow the guideline above. The equation is
P1/T1 = P2/T2.
Solve for P2 but substitute the numbers first and solve it step by step.
ok so 170/298=P2/333
which is .570...how do i find P2
ok so 170/298=P2/333
which is .570...how do i find P2
170/298 = P2/333
0.570 = P2/333
P2 = 0.570 x 333 = ?? atm.
To calculate the new pressure in the scuba tank, we can use the ideal gas law, which states that the product of the pressure (P) and volume (V) of a gas is equal to the number of moles (n) multiplied by the gas constant (R) and temperature (T). The formula for the ideal gas law is:
PV = nRT
Where:
P = pressure (in this case, in atmospheres)
V = volume (constant for a sealed scuba tank)
n = number of moles of gas (constant for a sealed scuba tank)
R = ideal gas constant (a constant value)
T = temperature (in Kelvin)
First, we need to convert the temperatures from degrees Celsius to Kelvin. The Kelvin temperature scale is used in the ideal gas law.
For the initial temperature:
T1 = 25°C + 273.15 = 298.15 K
For the final temperature:
T2 = 60°C + 273.15 = 333.15 K
Since the initial and final volume and the number of moles remain constant, we can rewrite the ideal gas law equation as:
P1 / T1 = P2 / T2
Where:
P1 = initial pressure (2500 psi)
P2 = final pressure (unknown, to be calculated)
Now, let's solve for P2 using the given values:
P2 / 298.15 K = 2500 psi / 333.15 K
To convert the pressure from psi to atmospheres, we need to know the conversion factor:
1 atmosphere = 14.7 psi
2500 psi / 14.7 psi/atm = P2 / 298.15 K
Simplifying further:
P2 = (2500 psi / 14.7 psi/atm) * (298.15 K / 333.15 K)
P2 ≈ 168.7 atm
Therefore, the new pressure in the scuba tank, when the temperature reaches 60°C, will be approximately 168.7 atmospheres.