Be sure to answer all parts. Hydrogen iodide decomposes according to the reaction 2 HI(g) ⇌ H2(g) + I2(g) A sealed 1.50−L container initially holds 0.00623 mol of H2, 0.00414 mol of I2, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H2(g) is 0.00467 M. What are the concentrations of HI(g) and I2(g)?

Answer : The concentration of and at equilibrium is, 0.0158 M and 0.00302 M respectively.

Explanation :

First we have to calculate the concentration of

Now we have to calculate the value of equilibrium constant (K).

The given chemical reaction is:

Initial conc.      0.0163     0.00415      0.00276

At eqm.        (0.0163-2x) (0.00415+x)  (0.00276+x)

As we are given:

Concentration of at equilibrium = 0.00467 M

That means,

(0.00415+x) = 0.00467

x = 0.00026 M

Concentration of at equilibrium = (0.0163-2x) = (0.0163-2(0.00026)) = 0.0158 M

Concentration of at equilibrium = (0.00276+x) = (0.00276+0.00026) = 0.00302 M

the answer is true. hope it .

it should have an internal chamber and two thermometers sticking out of the top. the internal chamber will also be closed off from the outside.