Final answer:
Using the ideal gas law PV = nRT and converting the given parameters to appropriate units, the temperature of the carbon dioxide is approximately 71.1 Kelvin.
Step-by-step explanation:
To calculate the temperature in Kelvin for 14.71 grams of carbon dioxide at a pressure of 196.1 kilopascals and a volume of 1200.0 milliliters, the ideal gas law can be used. The ideal gas law is expressed as 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.
Firstly, the number of moles (n) of CO2 needs to be calculated using its molar mass (about 44.01 g/mol). n = mass/molar mass = 14.71 grams / 44.01 g/mol ≈ 0.334 moles.
Next, we convert the volume from milliliters to liters since the standard unit for volume in the ideal gas law is liters (L). 1200.0 milliliters is equivalent to 1.200 liters.
The value for R (ideal gas constant) when pressure is measured in kilopascals and volume in liters is 8.314 L·kPa/mol·K.
Now we can rearrange the ideal gas law to solve for T:
T = PV/(nR)
T = (196.1 kPa * 1.200 L) / (0.334 mol * 8.314 L·kPa/mol·K)
T ≈ 71.1 Kelvin