Answer:
5.00 mol of an ideal gas will occupy 103.6 L at 25.0 C and 153 kPa of pressure.
Step-by-step explanation:
Using the ideal gas law, PV=nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the gas constant, and T is the temperature in Kelvin, we can solve for V.
First, we need to convert the temperature from Celsius to Kelvin by adding 273.15 K. Therefore, the temperature is 25.0 + 273.15 = 298.15 K.
Next, we can plug in the values we know:
PV = nRT
(153 kPa) V = (5.00 mol) (8.31 J/mol*K) (298.15 K)
Simplifying:
V = (5.00 mol) (8.31 J/mol*K) (298.15 K) / (153 kPa)
V = 103.6 L
Therefore, 5.00 mol of an ideal gas will occupy 103.6 L at 25.0 C and 153 kPa of pressure.