Describe the relative position of the equilibrium if Keq = 1.76 x 10-5

Consider the following reaction at equilibrium in the gas phase: N2   +   3 H2   double arrows   2 NH3 + heat In which direction will the equilibrium shift if the reaction is cooled?     Towards reactants     Towards products     Neither

According to Le Châtelier's principle, how will an increase in concentration of a reactant affect the equilibrium system?  Shift it toward the products  Shift it toward the reactants  Shift it toward the side with higher total mole concentration or  Shift it toward the side with lower total mole concentration

Acetaldehyde (CH3CHO) is an important chemical both industrially and biologically.  For instance, it is a (somewhat toxic) intermediate in the body's metabolism of ethanol into acetic acid, and thus is possibly implicated in the "hungover" symptoms of someone who has had too much to drink the night before.  In aqueous solution, it establishes an equilibrium with a hydrated form, shown below. CH3CHO (aq)   +   H2O (l)   <-->  CH3CH(OH)2 (aq) You start with an aqueous sample, already at equilibrium, with the CH3CH(OH)2 (the hydrated form) at a concentration of 2.60 M.  You have no information about how much, if any, of the anhydrous form (CH3CHO) is initially in the flask.  If you add 2.0 M of CH3CHO to the reaction flask, and as the equilibrium is being restored the amount of CH3CH(OH)2 changes by 1.13 M, what is the final amount of CH3CHO?

Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²

K = 1.3 \times 10-10 for the reaction HC6H50(aq) = H+(aq) + C6H50-(aq). In which direction is the equilibrium favored? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a Forward b Reverse c Appreciable quantities of all species are present at equilibrium d No direction is favored e There is not enough information to determine the direction

true or false

For the following reaction 2 SO2(g) + O2(g)   <->   2 SO3(g)  +  heat If the equilibrium situation is stressed by increasing the volume of the container, the reaction will shift toward a No change b Right or products c Left or reactants

Consider a reaction A21g2 + B21g2 ∆ 2 AB1g2, with atoms of A shown in red in the diagram and atoms of B shown in blue. (a) If Kc = 1, which box represents the system at equilibrium?

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease   (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease  (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e)…