Final answer:
To find the pressure in a 5.00 L tank with 10.00 grams of oxygen at 350 K, the number of moles of oxygen is first calculated and then substituted into the Ideal Gas Law equation, with the calculation resulting in the pressure in atmospheres (atm).
Step-by-step explanation:
To calculate the pressure of oxygen gas in a 5.00 L tank at 350 K, we will use the Ideal Gas Law formula, which is PV = nRT. Here, P is the pressure we need to find, V is the volume (5.00 L), n is the number of moles of gas, R is the ideal gas constant (0.08206 L · atm · mol⁻¹ · K⁻¹), and T is the temperature in Kelvin (350 K).
Firstly, we calculate the moles of oxygen gas. Oxygen has a molar mass of approximately 32 g/mol, so 10.00 grams of oxygen is 10.00 g / 32 g/mol = 0.3125 mol. Now that we have the number of moles, we can rearrange the Ideal Gas Law to solve for pressure: P = nRT / V.
Substituting the values we have, the calculation will be: P = (0.3125 mol)(0.08206 L · atm · mol⁻¹ · K⁻¹)(350 K) / (5.00 L).
The units of moles and liters will cancel out, leaving us with the pressure in atmospheres.
The pressure is 1.795 atm.