Final answer:
The pressure exerted by 25.0 g of CO₂ at a temperature of 25°C and a volume of 500 mL is approximately 3.45 atm.
Step-by-step explanation:
To find the pressure exerted by 25.0 g of CO₂, we need to use the ideal gas law equation, which states that 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 mass of CO₂ into moles. 25.0 g of CO₂ corresponds to approximately 0.568 moles of CO₂ (using the molar mass of CO₂). Next, we plug in the values into the ideal gas law equation: P(500 mL) = (0.568 moles)(0.0821 L·atm/K·mol)(25°C + 273 K). Rearranging the equation, we find that the pressure P is approximately 3.45 atm.