To find the pressure exerted by 25.0 g of CO2 at a temperature of 25.0°C and a volume of 500.0 mL, we can use the ideal gas law:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, we need to convert the given temperature from Celsius to Kelvin by adding 273.15:
T = 25.0°C + 273.15 = 298.15 K
The molar mass of CO2 is 44.01 g/mol. To find the number of moles, we divide the mass by the molar mass:
n = m/M = 25.0 g / 44.01 g/mol ≈ 0.568 mol
Now we can plug in the given values and solve for P:
P = (nRT) / V = (0.568 mol x 0.0821 L atm mol^-1 K^-1 x 298.15 K) / 0.500 L
P = 22.6 atm
Finally, we can convert the pressure from atm to Torr by multiplying by 760:
P = 22.6 atm x 760 Torr/atm ≈ 17176 Torr
Therefore, the pressure exerted by 25.0 g of CO2 at a temperature of 25.0°C and a volume of 500.0 mL is approximately 17176 Torr.