At a certain temperature, 0.3011 mol of N2 and 1.721 mol of H2 are placed in a 2.00 L container.   N2(g)+3H2(g)↽−−⇀2NH3(g) At equilibrium, 0.1401 mol of N2 is present. Calculate the equilibrium constant, ?c.

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Suppose a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1, (g) = BIOC1(g) + BrC1(g) The equilibrium constant K for this reaction is 4.15 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. 0.53 M ?

Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.1 mol of NH,. This reaction becomes possible: N, (g) +3H,(g) =2NH, (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 N,. You can leave out the M symbol for molarity. olo Ar N2 H, NH, initial change equilibrium 미

Suppose a 250. mL flask is filled with 1.6 mol of CH, 1.8 mol of H,O and 0.70 mol of CO. This reaction becomes possible: () +H,0(g) C0(g) +3H,(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 CO. You can leave out the M symbol for molarity. CH, H,0 CO H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use| Privacy I Accessibility 口ロ X

At a certain temperature, 0.317 mol CH, and 0.834 mol H,O is placed in a 3.00 L container. CH, (g) + 2 H,O(g) – CO,(g) + 4 H, (g) At equilibrium, 5.90 g CO, is present. Calculate K..

Suppose a 250. mL flask is filled with 0.20 mol of Cl,, 1.0 mol of CHCI, and 2.0 mol of CCI,. The following reaction becomes possible: Cl, (g) +CHCI, (g) HC1(g)+CCl,(g) The equilibrium constant K for this reaction is 8.66 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. IM

Suppose a 500. mL flask is filled with 0.90 mol of NO, and 1.8 mol of NO,. The following reaction becomes possible: NO, (g) +NO(g) - 2NO, (g) The equilibrium constant K for this reaction is 5.58 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. ©2022 McGraw Hill LLC. All Rights Reserved. Terms 43,203 FEB 19 PP ESS MacBook Air

Suppose a 250. mL flask is filled with 1.0 mol of CO, 0.60 mol of NO and 1.3 mol of CO2. The following reaction becomes possible: NO,(g) + CO (g) = NO(g)+CO,(g) The equilibrium constant K for this reaction is 3.67 at the temperature of the flask. Calculate the equilibrium molarity of NO,. Round your answer to two decimal places. ? Check Explanation

At a certain temperature, 0.960 mol SO, is placed in a 2.50 L container. 2 SO, (g) = 2 SO,(g) + 0,(g) At equilibrium, 0.190 mol O, is present. Calculate K. K. =