Final answer:
To calculate the temperature in oC for 1.02 moles of carbon dioxide in a 2,623 mL container at a pressure of 497.7 kPa, we can use the ideal gas equation. After converting the volume and pressure to appropriate units, we can substitute the values into the equation and solve for temperature. The temperature is approximately -144.66 oC.
Step-by-step explanation:
To calculate the temperature in oC for 1.02 moles of carbon dioxide in a 2,623 mL container at a pressure of 497.7 kPa, we can use the ideal gas equation:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the volume to liters and the pressure to atmospheres:
V = 2623 mL * (1 L / 1000 mL) = 2.623 L
P = 497.7 kPa * (1 atm / 101.325 kPa) = 4.905 atm
Now we can rearrange the equation to solve for T:
T = (PV) / (nR)
Substituting the given values:
T = (4.905 atm * 2.623 L) / (1.02 mol * 0.08206 L atm/(K mol))
T ≈ 128.49 K
Now we convert the temperature from Kelvin to degrees Celsius:
T (°C) = T (K) - 273.15
T (°C) ≈ 128.49 - 273.15
T (°C) ≈ -144.66 oC