Suppose a 500.mL flask is filled with 0.10mol of Cl2, 0.40mol of HCl and 0.80mol of...

Question

Question

Suppose a 500.mL flask is filled with 0.10mol of Cl2, 0.40mol of HCl and 0.80mol of CCl4. The following reaction becomes possible:

+Cl2gCHCl3g +HClgCCl4g

The equilibrium constant K for this reaction is 0.116 at the temperature of the flask.

Calculate the equilibrium molarity of HCl. Round your answer to two decimal places.

Answer 1

Answer #1

feakin uhl prted, bae huward divreins At o.1mole o.Inale .8mol 0.S AL 0.7- 0.1 +h mal mut. Mub CHGI CCA9 0.1- у о. 9- и orsy

Answer 2

Similar Homework Help Questions

Suppose a 500.mL flask is filled with 0.10mol of NO and 1.2mol of NO2. The following...

Suppose a 500.mL flask is filled with 0.10mol of NO and 1.2mol of NO2. The following reaction becomes possible: +NO3gNOg 2NO2g The equilibrium constant K for this reaction is 0.541 at the temperature of the flask. Calculate the equilibrium molarity of NO2. Round your answer to two decimal places
Suppose a 500. mL flask is filled with 1.9 mol of Cl2, 0.70 mol of HCl...

Suppose a 500. mL flask is filled with 1.9 mol of Cl2, 0.70 mol of HCl and 1.7 mol of CCI4. The following reaction becomes possible Cl2(g)+ CHCI3)HCI (g)+CCI4g) The equilibrium constant K for this reaction is 7.09 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places
Suppose a 250.mL flask is filled with 1.0mol of NO2 , 0.40mol of CO and 0.10mol...

Suppose a 250.mL flask is filled with 1.0mol of NO2 , 0.40mol of CO and 0.10mol of CO2 . The following reaction becomes possible: +NO2gCOg +NOgCO2g The equilibrium constant K for this reaction is 7.16 at the temperature of the flask. Calculate the equilibrium molarity of NO2 . Round your answer to two decimal places.

Suppose a 500.mL flask is filled with 0.50mol of H2 and 0.70mol of HCl. The following...

Suppose a 500.mL flask is filled with 0.50mol of H2 and 0.70mol of HCl. The following reaction becomes possible: H2g+Cl2g -> 2HClg The equilibrium constant K for this reaction is 1.17 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.
Suppose a 250. mL. flask is filled with 1.8 mol of Cl2 and 0.60 mol of...

Suppose a 250. mL. flask is filled with 1.8 mol of Cl2 and 0.60 mol of HCl. The following reaction becomes possible: H(+Cl()2HCI) The equilibrium constant K for this reaction is 8.25 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
Suppose a 500. ml flask is filled with 1.2 mol of Cl, and 0.80 mol of...

Suppose a 500. ml flask is filled with 1.2 mol of Cl, and 0.80 mol of HCl. The following reaction becomes possible: H2(g) + Cl2(g) = 2HCl (g) The equilibrium constant K for this reaction is 0.419 at the temperature of the flask. Calculate the equilibrium molarity of Cl. Round your answer to two decimal places. xs ?

Suppose a 500.mL flask is filled with 0.60mol of H2 and 0.70mol of Cl2. The following reaction becomes possible: H2(g) +...

Suppose a 500.mL flask is filled with 0.60mol of H2 and 0.70mol of Cl2. The following reaction becomes possible: H2(g) + Cl2(g) 2HCl(g) The equilibrium constant K for this reaction is 5.52 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 0.10 mol of Cl2 and 1.4 mol of...

Suppose a 250. mL flask is filled with 0.10 mol of Cl2 and 1.4 mol of HCl. The following reaction becomes possible: H2(g)+Cl2(g)=2HCl(g) The equilibrium constant for this reaction is 0.414 at the temperature of the flask. Calculate the equilibrium molarity of . Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 1.3 mol of H2 and 0.10 mol of...

Suppose a 500. mL flask is filled with 1.3 mol of H2 and 0.10 mol of HC1. The following reaction becomes possible: H2(g) + Cl2(g)-2HCl (g) The equilibrium constant K for this reaction is 3.03 at the temperature of the flask. Calculate the equilibrium molarity of H2. Round your answer to two decimal places.

Suppose a 500. ml flask is filled with 1.7 mol of Cl, and 2.0 mol of...

Suppose a 500. ml flask is filled with 1.7 mol of Cl, and 2.0 mol of HCl. The following reaction becomes possible: H2(g) +C12(g) + 2HCl (8) The equilibrium constant K for this reaction is 7.05 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. x o ?