Worksheet: Equilibrium Constants and Concentrations
In this worksheet, we will practice converting between equilibrium constant expressions and the concentrations of reactants and products.
Carbon monoxide and water react at high temperature according to the shown equation. Under certain conditions, the equilibrium constant for this reaction () is 5.0.
An equilibrium mixture of the substances was found to contain 0.20 mol of , 0.30 mol of water vapor, and 0.90 mol of per liter of gas. How many moles of were present in the equilibrium mixture?
Additional was added to the system at the same temperature, and some water vapor was removed by drying. A new equilibrium mixture was thereby established containing 0.40 mol of , 0.30 mol of water vapor, and 1.2 mol of per liter of gas. How many moles of were there in the new equilibrium mixture?
Antimony pentachloride decomposes according to the following equation. An equilibrium mixture in a 5.00 L flask at contains 3.85 g of , 9.14 g of , and 2.84 g of . How many grams of antimony pentachloride would be present if this mixture were transferred into a 2.00 L flask at the same temperature?
Sucrose is hydrolyzed to fructose and glucose according to the equation.
This reaction follows a first-order rate law. The products are structural isomers, exhibiting the same structural formula .
In neutral solution, = s−1 at . In the human body, the rate of this reaction is catalyzed by an enzyme, increasing the rate constant to at . What is the concentration of fructose after a 0.150 M aqueous solution of sucrose has reached equilibrium?
Gaseous nitrogen dioxide forms dinitrogen tetroxide according to the following equation. When 0.10 mol is added to a 1.0 L flask at , the concentration changes so that, at equilibrium, and .
What is the value of the reaction quotient before any reaction occurs?
What is the value of the equilibrium constant for the reaction?
Iodine molecules react reversibly with iodide ions to produce triiodide ions, as shown. Before a reaction, the concentrations of and in a solution are both equal to M. At equilibrium, the concentration of is M. If the concentrations of all species are 1.000 M under standard conditions, calculate the equilibrium constant for this reaction.
Ethanol and acetic acid react to form water and ethyl acetate, the solvent responsible for the odor of some nail polish removers, as shown. When 1.00 mol of each of and are allowed to react in 1.00 L of the solvent dioxane, equilibrium is established when mol of each of the reactants remains. What is the equilibrium constant, , for the reaction?
Acetic acid, , reacts with ethanol, , to form water and ethyl acetate, , as shown. The equilibrium constant for this reaction in dioxane is 4.0. A dioxane solution contains 0.15 M acetic acid, 0.15 M ethanol, 0.40 M ethyl acetate, and 0.40 M water when initially prepared. Calculate the concentration of ethyl acetate at equilibrium.
Consider the shown equilibrium.
A 1.00 L flask is filled with 1.00 mole of and 2.00 moles of . The value of the equilibrium constant for the reaction of hydrogen and iodine reacting to form hydrogen iodide is 50.5 under the given conditions. Calculate the equilibrium concentration of in the 1.00 L flask.
The equilibrium constant, , of a process may change if it is calculated relative to different standard conditions. For which process does the choice of standard conditions have no effect on ?