1. Convert grams of CH4 to moles:
* Molar mass of CH4 = 12.01 g/mol (C) + 4 * 1.01 g/mol (H) = 16.05 g/mol
* Moles of CH4 = 743.3 g / 16.05 g/mol = 46.32 mol
2. Use the Ideal Gas Law:
* The ideal gas law is: PV = nRT
* P = pressure (in atmospheres)
* V = volume (in liters)
* n = number of moles
* R = ideal gas constant (0.0821 L·atm/mol·K)
* T = temperature (in Kelvin)
3. Solve for Pressure (P):
* P = (nRT) / V
* P = (46.32 mol * 0.0821 L·atm/mol·K * 145.7 K) / 0.850 L
* P ≈ 837 atm
Therefore, the pressure exerted by 743.3 g of CH4 in a 0.850 L steel container at 145.7 K is approximately 837 atm.
