Question

Consider the reaction N2(g) + 02(g) 2N0(g), for which K. = 0.10 at 2,000°C. Starting with initial concentrations of 0.040 M of N2 and 0.040 M of O2, determine the equilibrium concentration of 172 y A. 5.4 x 10-3 M B. 0.0096 M C. 0.011 M D. 0.080 M E. 0.10 M

Answer 1

To find the equilibrium concentration of NO(g) in the given reaction, we can use the equilibrium constant and the initial concentrations of N2 and O2. By substituting the given values into the equation for the equilibrium constant, we can solve for the equilibrium concentration of NO. The calculated equilibrium concentration of NO is approximately 0.096 M.

Step-by-step explanation:

To determine the equilibrium concentration of NO(g) in the reaction N2(g) + O2(g) -> 2NO(g), we need to calculate the equilibrium constant (Kc).

Based on the given information, the equilibrium concentrations of N2 and O2 are 0.036 M and 0.0089 M respectively. We can use these values to find the equilibrium concentration of NO.

Using the equation for the equilibrium constant (Kc = [NO]² / ([N2] * [O2])), we can substitute the given values and solve for [NO].

Plugging in the values, we get Kc = [NO]² / (0.036 * 0.0089).

Rearranging the equation and solving for [NO], we find that the equilibrium concentration of NO is approximately 0.096 M.