Suppose a 500. mL flask is filled with 1.5 mol of H, and 1.0 mol of HCI. The following reaction becomes possible: H,(g) + Cl,(g) - 2HCI (g) The equilibrium constant K for this reaction is 0.348 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places.

Suppose a 500. mL flask is filled with 1.6 mol of N, and 0.10 mol of O,. The following reaction becomes possible: N,(g) +0,(g) 2NO(g) The equilibrium constant K for this reaction is 2.74 at the temperature of the flask. Calculate the equilibrium molarity of N,. Round your answer to two decimal places. 2:

Suppose à 250. mL flask is filled with 1.3 mol of CO, 1.8 mol of H,O and 1.6 mol of H,. This reaction becomes possible: co() +H,0(g) =CO,e)+H,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H,. You can leave out the M symbol for molarity. CO H,0 Co, H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Roserved Terms of Use Privacy 1 Ace O Type here to search

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -2 N2(g) + 3 H,(g) 2 NH3(g) K,=4. x 10 He fills a reaction vessel at this temperature with 9.0 atm of nitrogen gas and 4.5 atm of hydrogen gas. Use this data to answer the questions in the table below. dla O yes Can you predict the equilibrium pressure of NH, using only the tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of NH, at right. ||atm Round your answer to 1 significant digit. Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Accessibility