Answer:
a. P = 182 atm
b. due to daviation from ideal gas behavior
Explanation:
Data Given:
amount of CO = 122g
Volume of CO = .400 L
Temperature of CO = -71.2°C
Convert the temperature to Kelvin
T = °C + 273
T = -71.2 + 273
T = 201.8 K
a. Calculate the pressure exerted by the CO(g) in this system using the ideal gas equation (P) = ?
Solution:
To calculate Pressure by using ideal gas formula
PV = nRT
Rearrange the equation for Pressure
P = nRT / V . . . . . . . . . (1)
where
P = pressure
V = Volume
T= Temperature
n = Number of moles
R = ideal gas constant = 0.08206 L.atm / mol. K
For this we have to know the mole of the gas and the following formula will be used
no. of moles = mass in grams / molar mass . . . . . . (2)
Molar mass of CO = 12 + 16 = 28 g/mol
Put values in equation 2
no. of moles = 122 g / 28 g/mol
no. of moles = 4.4 mol
Now put the value in formula (1) to calculate Pressure for CO
P = 4.4 x 201.8 K x 0.08206 (L.atm/mol. K) / 0.400 L
P = 182 atm
So the pressure will be 182 atm
__________
b. Data Given:
Actual pressure exerted by CO = 145 atm
expected pressure exerted by CO = 182 atm
why the actual pressure is less than what would be expected = ?
Explanation:
This is because of the deviation from ideal behavior of real gases.
The real gases approaches to ideal behavior under very high temperature and very low pressure.
But CO deviate from ideal behavior to give expected value for pressure, because it behave at high pressure and low temperature.
This non-ideal behavior is due to two postulate of ideal behavior
• gas molecules have negligible volume
• Gas molecules have negligible inter-molecular interaction
but these postulates not obeyed under real condition. so we calculated the pressure using ideal condition values for gas and obtained the expected value for pressure but the actual pressure value was detected under normal condition.
