Final answer:
To determine the pressure of carbon monoxide in the container, the Ideal Gas Law is applied using the given number of moles, volume, and temperature, with the calculations revealing that the pressure is 7.15 atm.
Step-by-step explanation:
To calculate the pressure of carbon monoxide (CO) in the container we can use the Ideal Gas Law, which is PV = nRT. In this formula, P is the pressure of the gas, V is the volume of the container, n is the number of moles of the gas, R is the universal gas constant, and T is the temperature in Kelvin.
First, we convert the temperature from Celsius to Kelvin: T(K) = 52.5 °C + 273.15 = 325.65 K.
The universal gas constant (R) is 0.0821 L·atm/(K·mol) when pressure is measured in atmospheres and volume in liters.
Plugging in the values we have:
- n = 8.26 mol
- V = 30.0 L
- T = 325.65 K
- R = 0.0821 L·atm/(K·mol)
Now calculate the pressure (P):
P = (nRT)/V
P = (8.26 mol × 0.0821 L·atm/(K·mol) × 325.65 K) / 30.0 L
P = 7.15 atm
The pressure of the carbon monoxide in the container is 7.15 atm.