A 0.236g sample of carbon dioxide, CO2, has a volume of 595mL and a pressure of 455mmHg . What is the temperature, in kelvins and degrees Celsius, of the gas?
what is the degrees in celsius
Use PV = nRT and solve for T, which will be in kelvin. Then
K = C + 273 to calculate C.
To find the temperature of the gas in degrees Celsius, we can use the Ideal Gas Law equation:
PV = nRT
Where:
- P is the pressure (455 mmHg in this case)
- V is the volume (595 mL in this case)
- n is the number of moles of the gas (which we can find by dividing the mass of the carbon dioxide by its molar mass)
- R is the ideal gas constant (0.0821 L·atm/mol·K)
First, we need to find the number of moles of CO2 in the sample. The molar mass of CO2 is 44.01 g/mol.
n = mass / molar mass = 0.236 g / 44.01 g/mol = 0.00536 mol
Now we can rearrange the Ideal Gas Law equation to solve for temperature:
T = PV / (nR)
T = (455 mmHg * 595 mL) / (0.00536 mol * 0.0821 L·atm/mol·K)
T = (270725 mmHg·mL) / (0.000439856 L·atm/mol·K) = 616,027 K
To convert Kelvin to degrees Celsius, subtract 273.15:
T_in_Celsius = 616,027 K - 273.15 = 615,753.85 °C
Therefore, the temperature of the gas is approximately 616,027 Kelvin or 615,753.85 degrees Celsius.