The pressure exerted by 0.57 moles of CO2 at a temperature of 25°C and a volume of 500 ml is 28 atm.
Step-by-step explanation:
According to ideal gas law,
PV = nRT
where P represents the pressure of a gas,
V represents the volume of a gas,
n represents the number of moles,
R represents the gas constant = 0.0821 L atm / mol K.
T represents the temperature of a gas.
Given V = 500 ml = 0.5 l, T = 25°C = 298 K, n = 0.57 mol
PV = nRT
P = nRT / V
= (0.57
0.0821
298) / 0.5
P = 28 atm.
The pressure of a gas is 28 atm.