In a 250mL Erlenmeyer flask, a 0.50 gram piece of dry ice is
allowed to completely sublime and the pressure goes from 0.95 to
2.06 atm at a temperature of 24 degrees Celsius. Calculate the Gas
Law Constant. I got ~0.693 as the constant.
I changed 250ml to L = 0.25 L
24 C = 297.15 K
I wasn't sure if I was right about the pressure, so I subtracted
0.95 from 2.06.
I used PV/nt = r
Thank you!
Initial pressure = 0.95 atm
Final pressure = 2.06 atm
pressure due to CO2 = 1.11 atm
Volume of CO2 = 0.25 L
mass of CO2 = 0.50 g
moles of CO2 = mass of CO2 / molar mass of CO2
moles of CO2 = (0.50 g) / (44.0 g/mol)
moles of CO2 = 0.011364 mol
Temperature = 297.15 K
R = (P * V) / (n * T)
R = (1.11 atm * 0.25 L) / (.011364 mol * 297.15 K)
R = 0.08218 L-atm/mol-K
Actual value of R is 0.082057 L-atm/mol-K
Hence the value obtained from calculations is very close to actual value
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