Assume 5 mol of N2 gas is confined in a 10 L container at 523 K. calculate the pressure of the gas in kilopascals and in atmospheres.
2174111 KPa or 21.47 atm
Use PV = nRT. Remember T is in Kelvin. P will be in atmospheres. Then convert.
1 atm = 101.325 kPa.
To solve this problem, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = Pressure of the gas
V = Volume of the container
n = Number of moles of the gas
R = Ideal Gas Constant (0.0821 L·atm/(mol·K) or 8.314 J/(mol·K))
T = Temperature in Kelvin
First, we need to convert the temperature from Celsius to Kelvin by adding 273.15:
Temperature in Kelvin:
T = 523 K
Next, we can substitute the given values into the equation:
PV = nRT
P * 10 L = 5 mol * 0.0821 L·atm/(mol·K) * 523 K
Now, let's solve for the pressure (P):
P = (5 mol * 0.0821 L·atm/(mol·K) * 523 K) / 10 L
P ≈ 214.7 atm
To convert the pressure to kilopascals (kPa), we can use the following conversion factor:
1 atm = 101.325 kPa
Therefore, the pressure in kilopascals:
P (kPa) = 214.7 atm * 101.325 kPa/atm
P ≈ 21,777 kPa
So, the pressure of the gas is approximately 214.7 atm and 21,777 kPa.