What is the volume of a 5 g sample of carbon dioxide gas at a temperature of 88.2 oC and a pressure of 786.1 mmHg?
What is the pressure exerted by 6.26 g of argon with a volume of 2177.5 mL at a temperature of 12oC?
Please note that, the number of mol of CO2 is:
5/ 44= 0.114 mol, since the atomic mass of CO2 is 44 a.m.u. (atomic mass units)
Furthermore the pressure is P = 786.1/760 = 1.034 atm.
Then I apply the equation of gases:
P*V = n*R*T
where P is the pressure, V is the volume, Tis the temperature in Kelvin (273+88.2=361.2 °K), n is the number of moles of our sample of CO2; so I can write:
V = (n*R*T)/P = (0.114 * 0.08206*361.2) / 1.034 = 3.27 liters.
Here, the numbers of mol of Ar, is:
Then I apply the equation of gases, and I get:
P = (n*R*T)/V = (0.1565*0.08206*285) / 2.1775 = 1.68 atm,
since T = 273+12 = 285 °K, and V = 2177.5 / 1000 = 2.1775 liters
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