Antimony pentachloride, SbCl5, decomposes according to the following equation: ← SbCl5(g) → SbCl3(g) +Cl(g) An equilibrium mixture in a 5.00 L flask at 448 °C contains [SbCl5] = 0.002575 M, [SbCl3] = 0.008014 M and [Cl2] = 0.008011 M 1.State the type of equilibrium in the reaction 2.Calculate the mass in grams of each species that will be found when the mixture is transferred into a 2.00 L flask at the same temperature.

Sorry i dont understand the question can you rephase it?

Given data,temperature, t = 230°c = 503 kconsider the chemical reaction,ch₃oh(l) + 1/2 o₂(g)  → ch₂o(g) + h₂o(l)calculate the enthalpy change for the reaction: δh⁰rxn =  σnδh⁰f(products) -  σmδh⁰f(reactants)substitute the values from the table: δh⁰rxn = { -115.9 + (-285.8)} - {0+(-238.7)}              = -163.0 kjcalculate the entropy change for the reaction.δs⁰rxn = (219 + 70) - (127.2 + 1/2 x 205.2) = 59.2 j/kconsider the expression for free energy: δg⁰rxn =  δh⁰rxn - t  δs⁰rxnsubstitute the values in the above equationδg⁰rxn = -163 x 10³ - (503 x 59.2)              = -192777.6 j              = -192.777 kj