Upload the answer to this question as an image. Show your working. Consider the equilibrium step in the preparation of nitrosyl chloride, NOCI. 2NO(g) + Cl2(g) = 2NOCI(g) At a temperature of 727°C the equilibrium constant for this reaction is 3.09 × 10². The concentration of reactants and products at a particular moment in time in the realtion mixture is given below. [NO] = 0.0620 mol L1, [Cl2] = 0.538 mol L1, [NOCI] = 0.838 mol L-1 (i) Calculate the reaction quotient, Q, at this particular time. (ii) State whether the system is at equilibrium. Justify your answer. (iii) If the system is not at equilibrium explain which way the system will move in order to reach equilibrium. Give a reason for your answer.

Upload the answer to this question as an image. Show your working. Consider the equilibrium step in the preparation of nitrosyl chloride, NOCI. 2NO(g) + Cl2(g) = 2NOCI(g) At a temperature of 727°C the equilibrium constant for this reaction is 3.09 × 10². The concentration of reactants and products at a particular moment in time in the realtion mixture is given below. [NO] = 0.0620 mol L1, [Cl2] = 0.538 mol L1, [NOCI] = 0.838 mol L-1 (i) Calculate the reaction quotient, Q, at this particular time. (ii) State whether the system is at equilibrium. Justify your answer. (iii) If the system is not at equilibrium explain which way the system will move in order to reach equilibrium. Give a reason for your answer.

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter7: Reaction Rates And Chemical Equilibrium

Section: Chapter Questions

Problem 7.81P

See similar textbooks

Similar questions

At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
The equilibrium constant, Kc, is 1.05 at 350 K for the endothermic reaction 2 CH2Cl2(g) CH4(g) + CCl4(g) Which of the diagrams for Question 111 represents an equilibrium mixture at 350 K? Diagrams for Question 111.
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=* H+(aq) + COf-(aq) Assuming that the reactions in both directions are elementary' processes: Write rate expressions for the forward and reverse reactions. Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
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?
An experimenter places the following concentrations of gases in a closed container: [NOBr] = 7.13 102 M, [NO] = 1.58 102 M. [Br2] = 1.29 102 M. These gases then react: 2NOBr(g)2NO(g)+Br2(g) At the temperature of the reaction, the equilibrium constant Kc is 3.07 104. Calculate the reaction quotient, Qc, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium. a Qc = 6.33 104; the concentration of NOBr decreases b Qc = 6.33 104; the concentration of NOBr increases c Qc = 1.58 104; the concentration of NOBr increases d Qc = 4.65 104; the concentration of NOBr decreases e Qc = 4.65 104; the concentration of NOBr increases
For the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations are [SO2] = 0.102, [O2] = 0.0132, and [SO3] = 0.184. The concentration of SO2 is suddenly doubled. Show that the forward reaction takes place to reach a new equilibrium.
Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5H9CH3) but with a different molecular structure. sssss The equilibrium constant has been estimated to be 0.12 at 25 C. If you had originally placed 0.045 mol of cyclohexane in a 2.8-L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established?
The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.
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?