To solve for the pressure, we can use the ideal gas law:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the mass of oxygen to moles. The molar mass of oxygen is 32 g/mol, so:
n = m/M = 10 g / 32 g/mol = 0.3125 mol
Next, we need to convert the temperature to Kelvin. We can do this by adding 273.15 to the Celsius temperature:
T = 50°C + 273.15 = 323.15 K
Now we can plug in the values we have into the ideal gas law:
PV = nRT
P(2.00 L) = (0.3125 mol)(0.08206 L·atm/mol·K)(323.15 K)
Solving for P, we get:
P = (0.3125 mol)(0.08206 L·atm/mol·K)(323.15 K) / (2.00 L)
P ≈ 4.98 atm
Therefore, the pressure in the container is approximately 4.98 atm, rounded to one decimal place.