To find the pressure in the cylinder, we can use the ideal gas law equation:
PV = nRT
where P is the pressure, V is the volume (36.0 L), n is the number of moles of gas, R is the ideal gas constant (0.0821 L*atm/(K*mol)), and T is the temperature in Kelvin (25°C = 298 K).
First, we need to find the number of moles of each gas present in the cylinder. We can use the molar mass of each gas to calculate this:
Number of moles of CO2 = mass of CO2 / molar mass of CO2 = 350 g / 44.01 g/mol = 7.954 mol
Number of moles of O2 = mass of O2 / molar mass of O2 = 805 g / 32.00 g/mol = 25.156 mol
Number of moles of N2 = mass of N2 / molar mass of N2 = 4880 g / 28.01 g/mol = 174.165 mol
Next, we can calculate the total number of moles:
Total number of moles = moles of CO2 + moles of O2 + moles of N2 = 7.954 mol + 25.156 mol + 174.165 mol = 207.275 mol
Now we can substitute these values into the ideal gas law equation to find the pressure:
P * 36.0 L = 207.275 mol * 0.0821 L*atm/(K*mol) * 298 K
P = (207.275 mol * 0.0821 L*atm/(K*mol) * 298 K) / 36.0 L
P = 14.073 atm
So, the pressure in the cylinder is 14.1 atm.
The correct answer is 4. 14.1 atm.