(1) For the given system at equilibrium, NH4HS(s) <-----> NH3(g) + H2S(g), the K value is 1.6x10^-4 at 24oC, when pressures are in atmospheres.
What is the minimum mass of solid NH4HS(s) that can be introduced into a 5.0 L evacuated container so that equilibrium will result?
(2) Carbon Tetrachloride (CCl4) was once commonly used as a fire extinguisher. However, at high temperatures, CCl4 reacts with oxygen to form two deadly gases, phosgene and Cl2, according to the following chemical equilibrium.
2CCl4(g) +O2(g) <----> 2COCl2(g) + Cl2(g)
at 500oC, 0.562 mol of O2 and an unknown amount of CCL4 was introduced into a 1.00 L reaction vessel. Once the system had reached equilibrium, there was 0.263 moles of Cl2 present. Calculate the initial amount of CCL4 that was admitted into the vessel. K for this reaction at 500oC is 2.00 mol/l
The Attempt at a Solution
1) My textbook says as long as some solid is present the amount is a constant and it will not effect the concentration of ions in solution so I believe the answer would be any amount greater then zero. It is a six mark question though so I believe that is not the correct answer.
2) not to sure on this one
so this would give me the ratio of the concentrations of COCl2 over CCl4 but they should be equal to one because of the stoichiometry shouldn't they?