5.88 moles of nitrogen and 16.2 moles of oxygen are mixed and heated at 2000C° until equilibrium is established ,11,28 moles of nitric oxide are formed . Calculate the value of equilibrium constant?
I'm assuming a closed system of some volume I'll call L.
.................N2 + O2 ==> 2NO
I.............5.88.....16.2...........0
C..............?.........?...............?
E..............?..........?..............11.28
So ? for 2NO = 11.28. Then 11.28/2 = 5.64 mols O2 and 5.64 mols N2 were used and the table can be redone this way.
.................N2 + O2 ==> 2NO
I.............5.88.....16.2...........0
C.........-.5.64.....-5.64........11.28
E..........0.240.....10.56.......11.28
Do you want Kc. Note that no volume is available so mols/L can't be calculated; however, the volume, whatever it is, cancels in the calculation. Therefore, write the Kc expression, substitute thre E values in mols, and solve for Kc. To be complete, I would substitute 11.28/L, 0.240/L, and 10.56/L for the molarities of each component. Post your work if you get stuck.
To calculate the equilibrium constant (K), you need to write the balanced chemical equation for the reaction.
The given information tells us that nitrogen (N2) and oxygen (O2) react to form nitric oxide (NO), and the reaction has reached equilibrium with 11.28 moles of NO.
The balanced chemical equation for this reaction is:
N2 + O2 ⇌ 2NO
In this equation, the stoichiometric coefficients are 1 for N2 and O2 and 2 for NO.
Now, we need to calculate the concentrations of N2, O2, and NO at equilibrium, as the equilibrium constant is the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients.
To calculate the concentrations, we divide the number of moles by the total volume of the system. However, since the reaction is carried out at a high temperature, the volume of gases changes significantly, so we cannot rely on the actual volume.
Instead, we use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Given that the temperature is 2000°C, we convert it to Kelvin by adding 273 to get 2273K.
Since the total number of moles of gas is given (5.88 moles of N2 + 16.2 moles of O2), we can calculate the partial pressures of the gases using the ideal gas law. We can assume the pressure remains constant during the reaction.
Now, you have the partial pressure of N2, P(N2), and the partial pressure of O2, P(O2), at equilibrium. You also know that the number of moles of NO at equilibrium is 11.28.
The equilibrium constant expression for this reaction is:
K = [NO]^2 / [N2] * [O2]
To calculate K, substitute the values into the equation:
K = (11.28^2) / (5.88 * 16.2)
Solving this equation will give you the value of the equilibrium constant (K).
The balanced chemical equation for the reaction is as follows:
N2(g) + O2(g) ⇄ 2NO(g)
Given:
Initial moles of N2 = 5.88 mol
Initial moles of O2 = 16.2 mol
Moles of NO formed at equilibrium = 11.28 mol
To find the equilibrium constant (K), we need to use the equilibrium expression:
K = [NO]^2 / [N2] · [O2]
First, let's calculate the concentrations at equilibrium. Since we know the initial moles and the moles formed at equilibrium, we can subtract the moles formed from the initial moles to get the moles remaining at equilibrium:
Moles of N2 at equilibrium = Initial moles of N2 - Moles of NO formed
= 5.88 mol - 11.28 mol (since 2 mol of NO is formed from 1 mol of N2)
= -5.4 mol (negative value indicates that N2 is completely consumed)
Moles of O2 at equilibrium = Initial moles of O2 - Moles of NO formed
= 16.2 mol - 11.28 mol (since 2 mol of NO is formed from 1 mol of O2)
= 4.92 mol
Since N2 is completely consumed, the concentration at equilibrium is 0 mol/L. Therefore, [N2] = 0.
Now, substitute the values into the equilibrium expression:
K = [NO]^2 / [N2] · [O2]
K = (11.28 mol)^2 / (0 mol) · (4.92 mol)
K = Infinity (since [N2] = 0, the equilibrium constant is infinite)
Therefore, the value of the equilibrium constant is Infinity.