How many moles of gas (to 1 decimal place, input value only), are contained in a 54.25 L vessel at a pressure of 173.6 kPa and temperature of 0.2 °C?

To solve this problem, we will use the ideal gas law equation, which is PV = nRT.

Where: P = pressure V = volume n = number of moles R = ideal gas constant T = temperature

Given: P = 173.6 kPa V = 54.25 L T = 0.2 °C

First, we need to convert the temperature from Celsius to Kelvin because the ideal gas law requires the temperature to be in Kelvin.

T(K) = T(°C) + 273.15 T(K) = 0.2 + 273.15 = 273.35 K

Next, we need to convert the pressure from kPa to atm because the value of R we are using is in atm.

1 atm = 101.325 kPa P(atm) = P(kPa) / 101.325 P(atm) = 173.6 / 101.325 = 1.713 atm

Now we can substitute P, V, R, and T into the ideal gas law equation and solve for n.

n = PV / RT R = 0.0821 L.atm/K.mol (this is a constant value)

n = (1.713 atm * 54.25 L) / (0.0821 L.atm/K.mol * 273.35 K) n = 2.9 moles

So, there are approximately 2.9 moles of gas in the vessel.