Answer :
Final answer:
Using the Ideal Gas Law, and considering that the combustion of Carbon produces equal moles of CO2, approximately 49.78 Liters of CO2 are produced when 24.0 g of Carbon (C) is burned at a pressure of 99.3 kPa and a temperature of 298K.
Explanation:
To calculate the volume of CO2 produced from burning 24.0 g of Carbon (C) in this case,
we need to apply the Ideal Gas Law equation:
PV=nRT
where
P is pressure
V is volume
n is number of moles
R is the gas constant
T is temperature
Firstly, we need to identify the amount of Carbon in moles. 24.0 g of C equates to 2 moles of C (Considering C's atomic mass is ≈12 g/mol). When fully burned, one mole of Carbon will produce one mole of CO2, hence 2 moles of C will produce 2 moles of CO2.
Now, considering the Ideal Gas Law, the value of R (Universal gas constant) when Pressure is in kPa and Volume in Liters is 8.31 L·kPa/K·mol.
Given in the question, P=99.3 kPa and T=298 K. We must solve for V, so rearranging the formula we get V = nRT/P.
Substituting our known values, we calculate V = (2 mol * 8.31 L·kPa/K·mol * 298 K) / 99.3 kPa, which gives an approximate volume of 49.78 L.
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