Suppose a 500. mL flask is filled with 1.1 mol of Cl,, 0.80 mol of HCl and 1.8 mol of CCI. The following reaction becomes possible Cl2(g)+ CHCI,(g) – HCI (g) + CCI,(g) The equilibrium constant K for this reaction is 0.851 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places.

At equilibrium, the concentration of N2 is 5.32x10-3 M, O2 is 3.28 x10-3 M and that of NO is 6.19 x10-6 M. Evaluate the equilibrium constant for this reaction.

If concentration of a substance is increased, does the equilibrium shift toward or away from that side of the reaction? If concentration of a substance is decreased, does the equilibrium shift toward or away from that side of the reaction? If temperature is increased, does the equilibrium shift toward the side that contains heat or away from the side that contains heat? If temperature is decreased, does the equilibrium shift toward the side that contains heat or away from the side that contains heat? When a reaction shifts due to stress, what is the reaction trying to reach?

1. The shape of boron trihydride, BH3, is 2. In an exothermic reaction, the potential energy of the products is than the potential energy of the reactants. 3. A system at equilibrium always has forward and reverse reaction rates which are 4. A solution at 25°C with a pOH of 3.45 has a pH of 5. When nitric acid is titrated to an end point by lithium hydroxide, two products are and O 6. The standard reduction potential table lists the Evalues of half-cell reactions measured in combination with the standard half-cell.

When heat is added to exothermic reactions the equilibrium shifts towards the products. True False

What is the percentage of HCl in the solution if the molarity is 0.268398000?  Assume the density of the solution is 1.00 g/mL.

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 25 L tank with 11. mol of carbon monoxide gas and 12. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 6.9 mol of carbon monoxide gas, 7.9 mol of water vapor and 4.1 mol of hydrogen gas. The engineer then adds another 3.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. mol

Calculate the equilibrium partial pressure of H2

If the equilibrium constant of a given reaction is 2.10, what is the equilibrium constant of its reverse reaction?

Which of the following statements is a true statement concerning a reaction that has reached a state of equilibrium? A system has reached equilibrium when the concentrations of reactants and products remain constant. A system has reached equilibrium when the reaction has stopped and no more products are formed. A system has reached equilibrium when the rate constant for the forward reaction equals the rate constant of the reverse reaction. A system has reached equilibrium when the concentrations of reactants and products correspond to the stoichiometric ratios determined by the balanced equation.