A 6.0-L flask contains 0.60 g at a temperature of 25°C. What is the pressure (in atm) inside the flask?
To find the pressure inside the flask, we can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure in atm
V is the volume in liters
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/mol·K)
T is the temperature in Kelvin
First, let's convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 25°C + 273.15 = 298.15 K
Next, we need to calculate the number of moles (n) using the given mass and molar mass:
n = mass / molar mass
The molar mass of is 14.01 g/mol.
n = 0.60 g / 14.01 g/mol ≈ 0.043 moles
Now we can substitute the values into the ideal gas law equation and solve for pressure (P):
P * V = n * R * T
Since we have the volume (V) as 6.0 L, we can rearrange the equation to solve for P:
P = (n * R * T) / V
Plugging in the values:
P = (0.043 mol * 0.0821 L·atm/mol·K * 298.15 K) / 6.0 L
Calculating that:
P ≈ 0.350 atm
Therefore, the pressure inside the flask is approximately 0.350 atm.
The flask contains 0.60 g OF WHAT????
n = grams/molar mass of the material.
Then PV = nRT