answer #4 and 5 ework 3.pdf (113 KB)Page <1> of 2If an equilibrium mixture of the three gases in a 17.8 L container at 350 K contains 0.41-CH₂Cl2 and 0.419 mol of CH4, what is the equilibrium concentration of CCl4?3. A student ran the following reaction in the laboratory at 657 K2 NH3(g) → N₂ (g) + 3 H₂ (g)When she introduced 0.0657 moles of NH3 (g) into a 1.00 L container, she found the equiconcentration of H2 (g) to be 0.0918 M. Calculate the equilibrium constant Kc.4. Consider the equilibrium reaction2 HI (g) →→→→→→H₂(g) + 12(g)Kc = 55.6 at 698 KA reaction mixture was found to contain 0.0412 M H2, 0.0408 M of 12 and 0.269 M of HI.Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium?5. Consider the equilibrium reaction2 HI (g)H₂(g) + 12(g)Kc = 55.6 at 698 KIf the initial concentration of HI is 2.63 M, what are the concentrations of all substances atequilibrium?HQNZXT

#4: The balanced equilibrium reaction is: 2HI(g) ↔ H2(g) + I2(g) ; Kc = 55.6 at 698 K In order to…

4. Consider the equilibrium reaction 2 HI(g) ← H₂(g) + 12(g) Kc = 55.6 at 698 K A reaction mixture was found to contain 0.0412 M H2, 0.0408 M of 12 and 0.269 M of HI. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium 5. Consider the equilibrium reaction 2 HI(g) ← H₂(g) + 12(g) If the initial concentration of HI is 2.63 M, what are the concentrations of all substances at equilibrium? Kc = 55.6 at 698 K

4. Consider the equilibrium reaction 2 HI(g) ← H₂(g) + 12(g) Kc = 55.6 at 698 K A reaction mixture was found to contain 0.0412 M H2, 0.0408 M of 12 and 0.269 M of HI. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium 5. Consider the equilibrium reaction 2 HI(g) ← H₂(g) + 12(g) If the initial concentration of HI is 2.63 M, what are the concentrations of all substances at equilibrium? Kc = 55.6 at 698 K

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

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-.
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
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?
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
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?
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?
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
7-40 Is there any change in conditions that change the equilibrium constant, K, of a given reaction?
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.