what pressure is exerted by 784.3g of CH4 in a 0.870 l steel container at 184.3 k I don't know how to start it or the formula
Use PV = nRT
n = grams/molar mass CH4
To find the pressure exerted by a gas in a container, you can use the ideal gas law formula. The formula is:
PV = nRT
Where:
P = pressure of the gas (what we want to find)
V = volume of the container (0.870 L in this case)
n = number of moles of the gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin (184.3 K in this case)
To get started, we need to find the number of moles (n) of CH4. We can calculate this using the molar mass of CH4, which is 16.04 g/mol.
n = mass / molar mass
n = 784.3 g / 16.04 g/mol
n ≈ 48.9 mol
Now we can substitute the known values into the ideal gas law equation:
PV = nRT
P * 0.870 L = 48.9 mol * 0.0821 L·atm/mol·K * 184.3 K
Now we can solve for P:
P = (48.9 * 0.0821 * 184.3) / 0.870
P ≈ 871.2 atm
Therefore, the pressure exerted by 784.3g of CH4 in a 0.870 L steel container at 184.3 K is approximately 871.2 atm.