Be sure to answer all parts.The equilibrium constant (K) for the formation of nitrosyl chloride, anorange-yellow compound, from nitric oxide and molecular chlorine2NO(g) + Cl2(g) = 2NOCI(g)is 4 x 10° at a certain temperature. In an experiment, 2.60 × 102 mole of NO, 2.40 × 103mole of Cl2,and 4.60 moles of NOCI are mixed in a 2.80–L flask.What is Q. for the experiment?х 10(Enter your answer in scientific notation.)In which direction will the system proceed to reach equilibrium?The reaction will proceed to the left.The reaction will proceed to the right.The reaction is at equilibrium.

Answered: Image /qna-images/answer/75ba5c5d-0d29-4eec-93f1-8a1388d15e2b.jpg

Be sure to answer all parts.The equilibrium constant (K) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine 2NO(g) + Cl2(g) =2NOCI(g) is 4 x 106 at a certain temperature. In an experiment, 2.60 × 10-2 mole of NO, 2.40 × 103 mole of Cl,, and 4.60 moles of NOCI are mixed in a 2.80–L flask. What is Q, for the experiment? x 10 (Enter your answer in scientific notation.) In which direction will the system proceed to reach equilibrium? The reaction will proceed to the left. The reaction will proceed to the right. The reaction is at equilibrium.

Be sure to answer all parts.The equilibrium constant (K) for the formation of nitrosyl chloride, an orange-yellow compound, from nitric oxide and molecular chlorine 2NO(g) + Cl2(g) =2NOCI(g) is 4 x 106 at a certain temperature. In an experiment, 2.60 × 10-2 mole of NO, 2.40 × 103 mole of Cl,, and 4.60 moles of NOCI are mixed in a 2.80–L flask. What is Q, for the experiment? x 10 (Enter your answer in scientific notation.) In which direction will the system proceed to reach equilibrium? The reaction will proceed to the left. The reaction will proceed to the right. The reaction is at equilibrium.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

See similar textbooks

Similar questions

Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
Write the expression for the equilibrium constant and calculate the partial pressure of CO2(g), given that Kp is 0.25 (at 427 C) for NaHCO3(s) NaOH(s) + CO2(g)