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.
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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 0.10mol of Cl2, 0.40mol of HCl and 0.80mol of...
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.
Suppose a 500. mL flask is filled with 0.50 mol of H2 and 1.9 mol of...
Suppose a 500. mL flask is filled with 0.50 mol of H2 and 1.9 mol of HI. The following reaction becomes possible: H2(g)+12g2HIg The equilibrium constant K for this reaction is 4.94 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 0.70 mol of H2 and 0.60 mol of...
Suppose a 500. mL flask is filled with 0.70 mol of H2 and 0.60 mol of HI. The following reaction becomes possible: -2H1(g) The equilibrium constant K for this reaction is 2.38 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 1.3 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 0.80 mol of CO, 0.90 mol of CO2 and...
Suppose a 500.mL flask is filled with 0.80 mol of CO, 0.90 mol of CO2 and 0.20mol of H2. The following reaction becomes possible: COg+H2Og--->CO2g+H2g The equilibrium constant K for this reaction is 6.70at the temperature of theflask.Calculate the equilibrium molarity of H2O. Round your answer to two decimal places.
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 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 ?
Suppose a 500. ml flask is filled with 0.10 mol of H, and 1.0 mol of...
Suppose a 500. ml flask is filled with 0.10 mol of H, and 1.0 mol of HCl. The following reaction becomes possible: H2(g) +C1, (g) = 2HCl(g) The equilibrium constant K for this reaction is 4.69 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. x 6 ?
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 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 0.50 mol of H2 and 1.9 mol of HI. The following reaction becomes possible: H2(g)+12g2HIg The equilibrium constant K for this reaction is 4.94 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 0.70 mol of H2 and 0.60 mol of HI. The following reaction becomes possible: -2H1(g) The equilibrium constant K for this reaction is 2.38 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 1.3 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 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 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 ?
Suppose a 500. ml flask is filled with 0.10 mol of H, and 1.0 mol of HCl. The following reaction becomes possible: H2(g) +C1, (g) = 2HCl(g) The equilibrium constant K for this reaction is 4.69 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. x 6 ?
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 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 ?
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