Consider the equilibrium system: 2 ICI(s) = 12(s) + Cl2(g) Which of the following changes will increase the total amount of Cl, that can be produced? Choose all that apply Removing some of the I2(s) Adding more lCI(s) Decreasing the volume of the container Removing the Cl2 as it is formed

An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00 L container. CO(g) + H₂O(g) CO₂(g) + H₂(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished? moles of CO₂: 0.054 Incorrect mol

Titanium(IV) dchloride decomposes to form titanium and chlorine, like this: TiCl4(1)→Ti(s)+2 Cl,(9) At a certain temperature, a chemist finds that a 4.9 L reaction vessel containing a mixture of titanium(IV) chloride, titanium, and chlorine at equilibrium has the following composition: compound amount TiCl, 3.63 g dlo Ti 3.66 g Cl, 2.77 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K 0 Explanation Check All Righes Reserved Terms of Use Pivacy Center Accessib P Type here to search A a Pm Sc T Y P R U DE K A. Alt Ctrl Alt alexa INALED B.

Suppose a 250. mL flask is filled with 0.10 mol of Br,, 1.7 mol of OC1, and 0.20 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1,(g) -BROC1 (g) + BrCl (g) The equilibrium constant K for this reaction is 0.343 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. | M