Final answer:
The pressure of 4.00 mol of carbon dioxide gas in a 150 L cylinder at 27°C is calculated using the ideal gas law and is found to be 0.656 atm.
Step-by-step explanation:
To calculate the pressure of 4.00 mol of carbon dioxide gas in a 150 L cylinder at 27°C, we can use the ideal gas law: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
First, convert the temperature from Celsius to Kelvin by adding 273.15, giving us T = 27 + 273.15 = 300.15 K.
Now, we can solve for P:
P = (nRT) / V
= (4.00 mol × 0.0821 L·atm/mol·K × 300.15 K) / 150 L
= (98.444 mol·K) / 150 L
= 0.656 atm (rounded to three significant figures)