Answer:
look below
Step-by-step explanation:
It is not clear from the information provided what the initial pressure of the hydrocarbon was or the moles of each gas present in the vessel. In order to solve for the partial pressure of O₂(g), we need to know the total pressure of the gas mixture, the temperature, and the moles of each gas present.
Assuming that the temperature and total pressure of the gas mixture are as stated, we can use the ideal gas law to solve for the partial pressure of O₂(g). The ideal gas law is given by the equation:
PV = nRT
where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature in Kelvin.
If we let X be the partial pressure of O₂(g), Y be the partial pressure of the hydrocarbon, and n1 and n2 be the number of moles of O₂(g) and the hydrocarbon, respectively, we can set up the following system of equations:
X + Y = 1.4 atm
n1R(127+273) = XV
n2R*(127+273) = Y*V
We can solve this system of equations to find the partial pressure of O₂(g). However, we need to know the values of n1, n2, and V in order to do so. Without this information, it is not possible to calculate the partial pressure of O₂(g).