A 1.5L sample of CO2 contains 3.0 moles of CO2. How many moles of CO2 are lost when the volume is reducted to 0.75L?
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A 1.5L sample of CO2 contains 3.0 moles of CO2. How many moles of CO2 are lost when the volume is reducted to 0.75L?
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Answer:
We can use the ideal gas law to solve this problem:
PV = nRT
where P is the pressure of the gas, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Since the amount of CO2 is constant, we can write:
P1V1 = nRT1
where P1 = the initial pressure, V1 = the initial volume, and T1 = the initial temperature.
We can solve for n:
n = P1V1 / RT1
Now we can use the new volume (V2 = 0.75 L) to find the new pressure (P2):
P1V1 / T1 = P2V2 / T2
Since the temperature is constant, we can simplify:
P1V1 = P2V2
P2 = P1V1 / V2
We can now use the ideal gas law again to find the number of moles at the new pressure and volume:
n = P2V2 / RT1
Substituting our values:
n = (P1V1 / V2) * V2 / RT1
n = P1V1 / RT1
So the number of moles of CO2 does not change when the volume is reduced to 0.75 L.
Explanation:
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