For an ideal gas, calculate the following quantities.
(a) The pressure of the gas if 0.135 mol occupies 207 mL at 35°C.
_____atm
(b) The temperature (in kelvins) at which 0.0260 mol occupies 3.00 L at 0.563 atm.
__________K
(c) The number of moles in 5.00 L at -2°C and 735 torr. Remember 1atm = 760 torr.
_________mol
(d) The volume occupied by 6.72 10-3 mol at 20.°C and a pressure of 1.77 kPa. Remember 1 atm = 101.325 kPa
__________L
a) PV = nRT
T = temperature = 273 + 35 = 308 K
P = nRT/V = (0.135*0.0821*308) / 0.207 = 3.41 / 0.207 = 16.5 atm
b)
PV = nRT
0.563*3.00 = 0.0260 * 0.0821 * T
1.689 = 0.00213 * T
T = 793.0 K
Therefore, temperature is 793.0 K
c)
PV = nRT
P = pressure = 735 torr = 0.967 atm
0.967*5.00 = n * 0.0821*271
4.835 = n * 22.2
n = 0.218 mole
Therefore, the number of moles = 0.218
d)
PV = nRT
P = 1.77 kPa = 0.0175 atm
V = ?
n = 6.72*10^-3 mole
T = 273 + 20 = 293 K
0.0175 * V = (6.72*10^-3) * 0.0821 * 293
0.0175 V = 161.7*10^-3
V = 9.26 L
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