Help O KINETICS AND EQUILIBRIUMCalculating equilibrium composition from an equilibrium constantSuppose a 500. mL flask is filled with 1.0 mol of CHC1,, 0.40 mol of HCl and 1.6 mol of CCl,. The following reaction becomes possible:3'Cl, (g) +CHCI, (g) - HCI(g) + CCl,(g)The equilibrium constant K for this reaction is 5.65 at the temperature of the flask.Calculate the equilibrium molarity of HCI. Round your answer to two decimal places.OM

We have to find the equilibrium concentration of HCL

Suppose a 500. mL flask is filled with 1.0 mol of CHC1,, 0.40 mol of HCl and 1.6 mol of CCl,. The following reaction becomes possible: Cl, (g) +CHCI, (g) = HCI(g) + CCI,(g) The equilibrium constant K for this reaction is 5.65 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. M

Suppose a 500. mL flask is filled with 1.0 mol of CHC1,, 0.40 mol of HCl and 1.6 mol of CCl,. The following reaction becomes possible: Cl, (g) +CHCI, (g) = HCI(g) + CCI,(g) The equilibrium constant K for this reaction is 5.65 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. M

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.98PAE

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