3.4 Ideal Gas Law (AP Chemistry)
Created by Ehan
PV=nRT
PV = nRT
Pressure * Volume = number of particles * Ideal gas constant (R) * Temperature/energy
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| Term | Definition |
|---|---|
| PV=nRT | PV = nRT Pressure * Volume = number of particles * Ideal gas constant (R) * Temperature/energy |
| Ideal Gas Constant: R = 0.008206 | R = 0.08206 (L * atm)/(mol * K) We use the Ideal Gas Constant in the equation (PV = nRT) when we're using volume (V) in liters (L), pressure (P) in atm, number of particles (n) in moles (mol), and temperature (T) in kelvin (K) |
| Ideal Gas Constant: R = 62.36 | R = 62.36 (L * Torr)/(mol * K) Ideal Gas Constant for volume as liters (L), pressure as Torr, number of particles (n) as moles (mol), and temperature (T) in kelvin (K) |
| PV/nT = R | Take the original formula: PV = nRT Divide both sides by n and T, We get PV/nT = R |
| n = PV/RT | Take our original thingy: PV = nRT Divide both sides by R and T, We get PV/RT = n |
| P1V1 = P2V2 | P1V1 = P2V2 Pressure times volume in one state should equal pressure times volume of another because as V increases, P decreases, so multiplying them should ideally produce the same result. P (pressure) and V (volume) are inversely related. |
| P1/T1 = P2/T2 | P1/T1 = P2/T2 As temperature/energry (T) increases, pressure increases. So pressure divided by energy/temperature at one state is equal to pressure divided by energy/temperature in another. Pressure and energry (P and T) have a direct relationship. |
| Increased volume (V) | Lowered pressure (P) Inverse relationship |
| Decreased volume (V) | Increased pressure (P) Inverse relationship |
| Increased number of particles (n) | Increased pressure (P) Direct relationship |
| Decreased number of particles (n) | Increased pressure (P) Direct relationship |
| Kelvin to Celsius (°K to °C) | °K = °C+273.15 |
| Celsius to Kelvin (°C to °K) | °C = K-273.15 |