How many liters are occupied by 1.05 mol of nitrogen at 198�C and 0.564 atm pressure?
Answer in units of L
PV = nRT
i'm not getting the right answer
To find the number of liters occupied by a certain amount of gas, we can use the ideal gas law:
PV = nRT
Where:
P = pressure in atm
V = volume in liters
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin
First, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
So, T(K) = 198°C + 273.15 = 471.15 K
Now we can substitute the values into the ideal gas law equation and solve for V:
V = (nRT) / P
Given:
n = 1.05 mol
P = 0.564 atm
T = 471.15 K
R = 0.0821 L·atm/(mol·K)
Substituting the values into the equation:
V = (1.05 mol * 0.0821 L·atm/(mol·K) * 471.15 K) / 0.564 atm
Calculating this expression:
V = 27.99 L
Therefore, 1.05 mol of nitrogen at 198°C and 0.564 atm pressure occupies approximately 27.99 liters.