130 cm cube of a gas r200 temperature Celsius exert a pressure of 750 mm Jupiter calculate its pressure if the volume increased to 150 cm Cube at 350 temperature Celsius
PV/T is constant, so you want P such that
P*150/(273+350) = 750*130/(273+200)
I'm still trying to understand what r200 and Jupiter have to do with the problem unless that r200 is a refrigerant and we have a new element, Jupiter, that fills the barometer. Well, Jupiter and Mercury are planets. Maybe?
To calculate the new pressure of the gas in a larger volume and higher temperature, we can use the ideal gas law equation: PV = nRT.
Here's how you can determine the new pressure:
1. Convert the initial temperature from Celsius to Kelvin:
T1 = 200°C + 273.15 = 473.15 K
2. Convert the initial volume from cm³ to liters:
V1 = 130 cm³ = 130/1000 = 0.13 L
3. Convert the final temperature from Celsius to Kelvin:
T2 = 350°C + 273.15 = 623.15 K
4. Convert the final volume from cm³ to liters:
V2 = 150 cm³ = 150/1000 = 0.15 L
5. Use the ideal gas law equation to find the number of moles of the gas:
PV = nRT
n = (PV) / (RT)
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in K)
To find the number of moles, we need to use the initial conditions to calculate the initial number of moles (n1) and then use the final conditions to calculate the final number of moles (n2).
Initial:
n1 = (P1 * V1) / (R * T1)
Final:
n2 = (P2 * V2) / (R * T2)
Since the number of moles remains constant, n1 = n2.
6. Rearrange the equation to solve for the final pressure (P2):
P2 = (n1 * R * T2) / V2
Substitute the known values:
P2 = (n1 * 0.0821 * 623.15) / 0.15
Remember to use the same number of moles (n1) as calculated in step 5.
Using this equation, you can calculate the final pressure of the gas in the given conditions.