Suppose a 250. mL flask is filled with 1.0 mol of Cl, and 1.8 mol of HCl. The following reaction becomes possible: H, (g) + Cl, (g) – 2HC1(g) The equilibrium constant K for this reaction is 5.89 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. olo OM

O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.9 mol of NO,, 0.10 mol of N0 and 1.7 mol of CO,. The following reaction becomes possible: 2' NO,(g)+CO(g) -NO(g)+CO,(g The equilibrium constant K for this reaction is 4.70 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M TRADIS Explanation Check 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Acces NOV 242 PAGES étv 4 MacBook Air II

Suppose a 500. mL flask is filled with 0.70 mol of Cl,, 1.4 mol of CHCI, and 0.50 mol of CCl,. The following reaction becomes possible: 3 Cl,(g)+ CHC1,(g) – HC1 (g)+ CCl,(g) 4 The equilibrium constant K for this reaction is 1.78 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. ||M

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2 CH,(g) = 3 H, (g) + C,H, (g) 8- = 2. × 10 He fills a reaction vessel at this temperature with 14. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H,, using only the tools yes x10 available to you within ALEKS? no ? If you said yes, then enter the equilibrium pressure of H, at right. atm Round your answer to 1 significant digit.

Suppose a 250. mL flask is filled with 0.20 mol of 0, and 1.4 mol of NO. The following reaction becomes possible: N,(g) + 0,(g) – 2NO(g) The equilibrium constant K for this reaction is 4.19 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. ?

Suppose a 500. mL flask is filled with 0.40 mol of N, and 0.10 mol of 0,. The following reaction becomes possible: N, (g) + 0,(g) – 2NO(g) The equilibrium constant K for this reaction is 5.29 at the temperature of the flask. Calculate the equilibrium molarity of N,. Round your answer to two decimal places. OM

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2CH₂(g) 3H₂(g) + C₂H₂(g) K,=3.x 108 He fills a reaction vessel at this temperature with 11. atm of methane gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of H₂, using only the tools yes available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of H₂ at right. Round your answer to 1 significant digit. at atm X

Suppose a 500. mL flask is filled with 0.30 mol of Cl, and 1.2 mol of HCl. The following reaction becomes possible: H,(g) +Cl, (g)- 2HC1(g) (3) 12+ The equilibrium constant K for this reaction is 5.59 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. |M