A sample of co2 gas at 90.7 degree celsius has a volume of 300. ml at 810 mmHg. How many moles of co2 are present R=.08206 L atm/mol K 1 atm=760 mmHg
Use PV = nRT
P must be in atm, T in kelvin, V in L.
is this correct?
(1.07)(0.3)=(44.01)(.08206)(363.7)
0.3424=1313.49
=0.00026068 or 2.61^-4
I responded to your second post above.
To determine the number of moles of CO2 present, we can use the Ideal Gas Law equation: PV = nRT, where P represents the pressure, V represents the volume, n represents the number of moles, R is the gas constant, and T represents the temperature in Kelvin.
First, let's convert the temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 90.7 + 273.15
T(K) = 363.85 K
Next, we need to convert the pressure from mmHg to atm:
P(atm) = P(mmHg) / 760
P(atm) = 810 / 760
P(atm) = 1.0658 atm
Now, we can rearrange the Ideal Gas Law equation to solve for the number of moles (n):
n = PV / RT
Plugging in the values:
n = (1.0658 atm) * (0.300 L) / [(0.08206 L atm / mol K) * (363.85 K)]
Calculating:
n = 0.3197 mol
Therefore, there are approximately 0.3197 moles of CO2 present in the given sample.