What is the pressure (in kPa) of a 0.055 mol sample of krypton gas that has a temperature of 188°C and a volume of 0.57 L?

Answer 1

We can use the ideal gas law equation, PV = nRT, where p is pressure, v is volume, n is mols, R is a gas constant (8.3145) and t is temperature.

We can rearrange the equation to solve for pressure: P = nRT/V

1. We were given n = 0.055 mol
2. We know the value of R (8.3145)
3. We were given T in celsius which we can convert to kelvin (just add 273.15): 188 + 273.15 = 461.15
4. We were given v = 0.57 L

We can now plug in all of these values: (P = 0.055 x 8.3145 x 461.15)/0.57 =369.97 Pa

We can convert to kPa, 369.97 x 10^-3 (final answer)