Answer:
8.214 liters.
Step by step explanation:
The ideal gas law is 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. To use this formula, we need to convert the temperature from Celsius to Kelvin by adding 273.15.
n = 0.25 mol
P = 0.82 atm
T = (57 + 273.15) K = 330.15 K
R = 0.08206 L·atm/(mol·K)
Plugging these values into the ideal gas law, we get:
V = nRT/P
V = (0.25 mol) x (0.08206 L·atm/(mol·K)) x (330.15 K) / (0.82 atm)
V = 8.214 L
Therefore, the volume of 0.25 mol of nitrogen at 0.82 atm pressure and 57 C temperature is approximately 8.214 liters.