Water gas is a mixture of carbon monoxide and hydrogen that is formed when carbon reacts with steam. C(s) + H₂O(g) CO(g) + H₂(g) Which of the changes below will affect the equilibrium of this system? Choose one or more: Adding coal to the reaction vessel Adding carbon monoxide to the reaction vessel Adding steam to the reaction vessel Adding a catalyst

For this reaction, the equilibrium constant, Kea, is 6.1 x 10-4 SO3 (g) - O2 (g) + 2SO3 (g) Select the most accurate statement. O the equilibrium favors reactants O the rate of the forwards reaction is very fastfast O at equilibrium, the reaction mixture will contain a lot of both reactants and products O the rate of the forwards reaction is very slow O the equilibrium favors products

Mercury(II) oxide decomposes to form mercury and oxygen, like this: 2 HgO(s)→2 Hg(1)+O2(g) At a certain temperature, a chemist finds that a 3.3 L reaction vessel containing a mixture of mercury(II) oxide, mercury, and oxygen at equilibrium has the following composition: compound amount HgO 19.5 g Hg 14.6 g O2 0, 17.4 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 x10

adding some CO(g) increasing the volume of the container removing some H₂O(g) Shifts in the direction of the products Shifts in the direction of the reactants chill the reaction removing H₂(g) as it forms Equilibrium does not change