Given information:
- A cylinder contains a gaseous mixture containing CO and N2.
- We need to find the ratio of their partial pressure in the cylinder.

Partial pressure of a gas:
The partial pressure of a gas in a mixture of gases is the pressure that gas would exert if it occupied the same volume alone at the same temperature.

Formula:
Partial pressure of a gas = mole fraction of that gas × total pressure of the mixture

Mole fraction of a gas:
The mole fraction of a gas in a mixture is the ratio of the number of moles of that gas to the total number of moles of all gases present in the mixture.

Formula:
Mole fraction of a gas = number of moles of that gas / total number of moles of all gases present in the mixture

Solution:
Let the partial pressure of CO be P_CO and the partial pressure of N2 be P_N2.
Let the mole fraction of CO be x_CO and the mole fraction of N2 be x_N2.

From the given information, we can write:
- The total pressure of the mixture = P_CO + P_N2
- The total number of moles of gases present in the mixture = n_CO + n_N2

We can also write:
- x_CO + x_N2 = 1 (since they are the only two gases present in the mixture)

Now, let's find the mole fraction of each gas:
- Mole fraction of CO:
x_CO = n_CO / (n_CO + n_N2)
We don't know the values of n_CO and n_N2, but we can use the ratio of their volumes to find their ratio of moles.
Assuming the cylinder is at standard temperature and pressure (STP), we know that 1 mole of any gas occupies 22.4 L of volume at STP.
Let's say the cylinder has a volume of V_L and contains V_CO L of CO and V_N2 L of N2.
Then, we can write:
V_CO / 22.4 = n_CO / 1
V_N2 / 22.4 = n_N2 / 1
Dividing the two equations, we get:
V_CO / V_N2 = n_CO / n_N2
So, the ratio of moles of CO to N2 is equal to the ratio of their volumes in the cylinder.
Let's say this ratio is k_CO:N2.
Then, we can write:
n_CO / n_N2 = k_CO:N2
Substituting this in the expression for x_CO, we get:
x_CO = k_CO:N2 / (1 + k_CO:N2)
- Mole fraction of N2:
x_N2 = n_N2 / (n_CO + n_N2)
Substituting the value of n_CO / n_N2 from above, we get:
x_N2 = 1 / (1 + k_CO:N2)

Now, let's find the partial pressures of each gas:
- Partial pressure of CO:
P_CO = x_CO × (P_CO + P_N2)
Substituting the value of x_CO from above, we get:
P_CO = k_CO:N2 × (P_CO + P_N2) / (1 + k_CO:N2)
- Partial pressure of N2:
P_N2 = x_N2 × (P_CO + P_N2)
Substit

Option A is correct...