Answer :
Final answer:
The student's question is a chemistry problem about the Ideal Gas Law. By converting the temperature to Kelvin and substituting the given values into the Ideal Gas Law equation (n = PV/RT), we find that approximately 13.4 moles of chlorine gas would be present.
Explanation:
The student's question is asking how many moles of chlorine gas at 110 degrees Celsius and 28.0 atm would occupy a vessel of 15.0 L.
This is a chemistry problem and can be solved using the Ideal Gas Law equation,
PV = nRT, where
P is the pressure,
V is the volume,
n is the number of moles,
R is the gas constant, and
T is the temperature in Kelvin.
In this problem, we are solving for n - the number of moles.
First, convert the temperature to Kelvin by adding 273.15 to the Celsius temperature (110 + 273.15 = 383.15 K).
Then rearrange the equation to solve for
n (n = PV/RT).
Substitute the given values into the equation
(n = (28.0 atm * 15.0 L) / (0.0821 L·atm/K·mol * 383.15 K).
This gives you an answer of approximately 13.4 mol.
Conclusion
Therefore, the main answer is (b) 13.4 mol. This corresponds to the amount of chlorine gas in moles that would occupy a 15.0 L vessel at a temperature of 110 degrees Celsius and a pressure of 28.0 atm.
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