Achemist wants to find kc for the following reaction at 751 k: 2nh3(g) + 3 i2 (g) latex: \longleftrightarrow ⟺ 6hi(g) + n2(g) kc = use the following data at 751 k to find the unknown kc: (1) n2(g) + 3 h2(g) latex: \longleftrightarrow ⟺ 2 nh3(g) kc1 = 0.282 (2) h2(g) + i2(g) latex: \longleftrightarrow ⟺ 2 hi(g) kc2 = 41 enter to 0 decimal places.

The equilibrium constant for the total reaction is

Explanation:

We are given:

We are given two intermediate equations:

Equation 1:

The expression of for the above equation is:

       .......(1)

Equation 2:

The expression of for the above equation is:

      ......(2)

Cubing both the sides of equation 2, because we need 3 moles of HI in the main expression if equilibrium constant.

Now, dividing expression 1 by expression 2, we get:

The above expression is the expression for equilibrium constant of the total equation, which is:

Hence, the equilibrium constant for the total reaction is

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)