Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the reactant concentrations drop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the product concentrations rise. At equilibrium all reactions stop. As a reaction proceeds forward toward equilibrium the forward rate constant drops.

Consider the following reversible reaction at equilibrium: CO(g) + Cl2(g) COCI,(g). Use Le Chatelier's principle to predict the effect of adding some Cl2(g) to the equilibrium system? the concentration of CO(g) increases the concentration of COC12(g) decreases the equilibrium system shifts to the right to restore equilibrium the equilibrium system shifts to the left to restore equilibrium no effect

Question 29 of 30 Consider the reaction of N2O and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. 2 NO(g) +3 O₂(g) 4 NO2(g) 1 2 NEXT > A 1.00 L reaction vessel was filled with 0.0560 mol O2 and 0.200 mol N2O and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. 2N₂O(g) + 302(g) == 4NO2(g) Initial (M) 0.200 -0.0100 0.190 Change (M) 0.0560 -0.0150 0.0410 Equilibrium (M) 0 0.0200 0.0200 RESET 0 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190

For the equilibrium shown below, assess whether the following mixture is at equilibrium.  If the mixture is NOT at equilibrium, tell whether the reaction will form more reactant or more products to reach equilibrium. 2 CO2 (g) 2 CO (g) + O2 (g) Kc = 6.4 x 10-7   [CO2] = 5.3 x 10-2 M   [CO]  = 3.6 x 10-4 M   [O2]    = 2.4 x 10-3 M

I Review | Constants | Periodic Table Part B When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K. The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: The following system is at equilibrium:A(s) + 4B(g) = C(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help If a stress is applied to a reaction mixture at equilibrium,…

Given the following reaction, the equilibrium constant, and the initial concentrations; answer the four bullet questions. 2 NO2 (g) - 2 NO (g) + O2 (g) Kc = 1.56 x 10-10 Initial Species Concentration (M) NO2 5.62 x 10-10 NO 3.99 x 10-16 O2 9.35 x 10-3 • Set up the equilibrium expression, and calculate the reaction quotient (Q). Note: ^ means "to the" Q = [ Select ] • How does Q compare to K? Q is [ Select]

The chemical equation represents a reaction at equilibrium. 2SO3(g) = 2SO2 (g) +O2(g) Which of these shows the equilibrium constant expression for this chemical equation? A [O2][SO2]2/[SO3]2 B [O2]2[SO2]/2[SO3] C 2[SO3]/[O2]2[SO2] D [SO3]2/[O2][SO2]2

True/False. Explain your answer in one sentence or less.   In an equilibrium process, the concentrations of products and of reactants are equal. The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants. Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point. The concentration of a pure solid is left out of an equilibrium constant expression but a pure liquid is included.

Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. At equilibrium the speed of a reaction equals its rate constant. At equilibrium concentrations of reactants and products stay constant. At equilibrium the reverse rate equals zero. ☐ At equilibrium the rate of change of product concentration is zero. As a reaction proceeds backwards toward equilibrium the product concentrations drop.