A system being studied in a 3.0-liter reactor was charged with 0.150 moles of H2, 0.150 moles of X2, and 0.600 moles of HX. A catalyst was introduced using a remote unit. Is the reaction at equilibrium

The reaction is not in equilibrium and it proceed in reverse direction to reach the equilibruim condition

Explanation:

We have

H₂(g) + x₂(g)  ⇆  2HX (g)

Kc = 2.4 x 10 ⁻³ at 25°C

Now we have 3L reactor and the number of mole of species are 0.150 mole H₂, 0.150 mole X₂ and 0.600 mole HX

Therefore,

Therefore,

Now, we calculate the free energy change for the reaction

ΔrG = RT In Q/K

As free energy is +ve so the reaction is not in equilibruim and proceed in reverse reaction to reach tje equilibruim condition

the answer is the

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.