Final answer:
To find the pressure of 5.6 moles of gas at a temperature of 285 Kelvin and a volume of 20.0 liters, we use the ideal gas law, which yields approximately 1.19 atm.
Step-by-step explanation:
To calculate the pressure (in atm) of 5.6 moles of a gas at a temperature of 285 Kelvin in a volume of 20.0 liters, we use the ideal gas law: PV=nRT. Here, P is the pressure, V is the volume, n is the number of moles, T is the temperature in Kelvin, and R is the ideal gas constant, which is 0.0821 (atm·L)/(mol·K) when pressure is in atmospheres.
Inserting the given values into the ideal gas law equation, we get:
P (20.0 L) = (5.6 mol) (0.0821 atm·L/mol·K) (285 K)
To solve for P, we calculate:
P = (5.6 mol × 0.0821 atm·L/mol·K × 285 K) / 20.0 L
P = 1.192924 atm
Therefore, the pressure of the gas in the given conditions is approximately 1.19 atm.