The instruction booklet for your pressure cooker indicates that its highest setting is 13.5psi . You know that standard atmospheric pressure is 14.7psi , so the booklet must mean 13.5psi above atmospheric pressure. At what temperature will your food cook in this pressure cooker set on "high"?
I tried: PV=nRT
V, n, R = constant
P = T
P1/T1 = P2/T2
P1=14.7psi
T1 = 20C
P2 = 14.7+13.5 psi
T2= ?
But I am not getting the correct value am I using the correct equation or should i be using ln(P1/P2)=change in heat vapor/R * (1/T2 - 1/T1)
Thanks
119 degrees celsius
you are using the wrong equation. Us the other one
To solve this problem, you need to use the ideal gas law equation, PV = nRT, where P represents pressure, V represents volume, n represents the number of moles, R is the ideal gas constant, and T represents temperature in Kelvin.
Since the pressure cooker operates at a pressure of 13.5 psi above atmospheric pressure, you need to convert the pressure to absolute pressure by adding the atmospheric pressure:
P2 = 14.7 + 13.5 = 28.2 psi
First, let's convert the pressures to the SI unit of pressure, which is Pascal (Pa):
P1 = 14.7 psi * 6894.76 Pa/psi = 101,775.72 Pa
P2 = 28.2 psi * 6894.76 Pa/psi = 194,247.12 Pa
Now let's convert the temperatures to Kelvin:
T1 = 20°C + 273.15 = 293.15 K
Now start by using the ideal gas law equation to solve for T2:
P1/T1 = P2/T2
Rearrange the equation to solve for T2:
T2 = (P2 * T1) / P1
Substituting the values we have:
T2 = (194,247.12 Pa * 293.15 K) / 101,775.72 Pa
Calculating this yields:
T2 ≈ 557.58 K
So, the temperature at which your food will cook in the pressure cooker set on "high" is approximately 557.58 Kelvin.