If 0.25 mol of methane gas (CH4) is introduced into evacuated 2.00 L container at 35 Degrees Celcius , what is the pressure in the container ?
See your post above.
To find the pressure inside the container, we can use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure of the gas (in units of pressure, such as atm)
V = volume of the container (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L.atm/(mol.K))
T = temperature of the gas (in Kelvin)
First, let's convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 35°C + 273.15 = 308.15 K
Now, we can plug in the values we have:
P * 2.00 L = 0.25 mol * 0.0821 L.atm/(mol.K) * 308.15 K
Let's solve for P:
P = (0.25 mol * 0.0821 L.atm/(mol.K) * 308.15 K) / 2.00 L
P ≈ 10.17 atm (rounded to two decimal places)
Therefore, the pressure inside the container is approximately 10.17 atm.