Which of the following describes a situation in which it can be safely assumed that the equilibrium concentration of a species is for all practical purposes equal to its initial concentration? O The K value for the reaction is large. O The initial concentrations are very small. O The K value for the reaction is nearly equal to 1. O The K value for the reaction is small.

Define equilibrium constant Keq

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature.  If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?

Consider the following equilibrium system: 2SO2 + O2 --> 2SO3 Into a 2.00 Liter container, 0.500 mol of SO3, was placed and heated to 300°C. After equilibrium was established, the container was found to have 0.300 moles of SO3 present along with the other gases. Calculate the equilibrium concentration of each molecule and the equilibrium constant for this reaction at this temperature.

Assume that the following endothermic chemical reaction is at equilibrium. C(s) + H₂O(g) + H₂(g) + CO(g) Which of the following statements is/are CORRECT? 1. Increasing the concentration of H₂(g) will cause the reaction to proceed in the backward direction, increasing the equilibrium concentration of H₂O(g). 2. Decreasing the temperature will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). 3. Increasing the amount of C(s) will cause the reaction to proceed in the forward direction, increasing the equilibrium concentration of CO(g). All statements are correct. 2 only 3 only 1 only 1 & 2 only

When a system is at equilibrium: the reaction rate of the forward reaction is small compared to the reverse. the amount of product and reactant is exactly equal. the reaction rate of the forward reaction is equal to the rate of the reverse. the reaction rate of the reverse reaction is small compared to forward.

A system is considered to be at equilibrium. Which statement must be true? a) The reaction has stopped. b) The products and reactants are now equal in concentration. c) The reaction equilibrium state cannot be altered. d) There is no net change in the amount of reactant or product.

What does it mean for a chemical reaction to reach equilibrium?         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are also equal.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are equal.         The rates of the forward and reverse reactions are equal. The concentrations of the reactants and products are constant.         The rates of the forward and reverse reactions are increasing. The concentrations of the reactants and products are also increasing.

Calculate the equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture.

Calculating an equilibrium constant from a partial equilibrium.. Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. An industrial chemist studying this reaction fills a 2.0 L flask with 3.9 atm of sulfur dioxide gas and 0.74 atm of oxygen gas, and when the mixture has come to equilibrium measures the partial pressure of sulfur trioxide gas to be 1.2 atm. Calculate the pressure equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. Round your answer to 2 significant digits. K, = [ %3D do x10 Ar Eplanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibility FEB tv 23 30 MacBook Air DII DD F12 F11 F10 F9 80 888 F8 F7 F5 F6 F4 F3 esc F2 F1 $ % @ 8. 3 4 5 6 2 U