Assume equilibrium exists for the reaction shown below. One of the statements regarding equilibrium is incorrect. Which one? H₂(g) + Cl₂(g) = 2HCl(g) O The rate of reaction H2 + Cl2 --> 2HCl equals the rate of reaction 2HCI --> H2 + C12 There is no observable change in the system as time evolves O The rate of the reaction H2 + C12 --> 2HCI is zero; that is, the reaction'does not occur The concentrations of H2, C12, and HCI stay constant

Assume equilibrium exists for the reaction shown below. One of the statements regarding equilibrium is incorrect. Which one? H₂(g) + Cl₂(g) = 2HCl(g) O The rate of reaction H2 + Cl2 --> 2HCl equals the rate of reaction 2HCI --> H2 + C12 There is no observable change in the system as time evolves O The rate of the reaction H2 + C12 --> 2HCI is zero; that is, the reaction'does not occur The concentrations of H2, C12, and HCI stay constant

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

= O KINETICS AND EQUILIBRIUM Using Le Chatelier's Principle to predict the result of changing... Acetylene and oxygen react to form carbon dioxide and water, like this: 2C₂H₂(g) +50₂(g) → 4CO₂ (g)+2H₂O(g) Suppose a mixture of C₂H₂, O₂, CO₂ and H₂O has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some H₂O is removed. Some C₂H, is added. change in composition The pressure of C₂H₂ will The pressure of O₂ will The pressure of O₂ will The pressure of CO₂ will ? ? ? ? ? V go up. go down. not change. shift in equilibrium O to the right to the left x O (none) 3/5 to the right to the left (none)
The reaction below was allowed to react at 375 degrees Celcius until it formed an equilibrium. At equilibrium, the 16.2 L container was found to contain 1.9 mol SiF4, 1.1 mol H2O, 3.5 mol SiO2, and 2.9 mol HF. What is the Kc of the reaction at this temperature? SiF4 (g) + 2H2O (g) <--> SiO2 (s) + 4HF(g)
The progress of the reaction H2(g) + Br2(g) 2 2 HBr(g) can be monitored visually by following changes in the color of the reaction mixture (Br2 is reddish brown, and H2 and HBr are colorless). A gas mixture is prepared at 700 K, in which 0.40 atm is the initial partial pressure of both H2 and Br, and 0.90 atm is the initial partial pressure of HBr. The color of this mixture then fades as the reaction progresses toward equilibrium. Give a condition that must be satisfied by the equilibrium constant K (for example, it must be greater than or smaller than a given number).
5. Study the following reactions: 2H2O2⇌2H2O+O22H2O2⇌catalyst2H2O+O2Reaction 1: uncatalyzedReaction 2: catalyzed If the two reactions occur at the same temperature, which statements are true? Select all that apply. The catalyzed reaction will reach equilibrium faster than the uncatalyzed reaction. The uncatalyzed reaction will reach equilibrium faster than the catalyzed reaction. The equilibrium position of the catalyzed reaction is greater than that of Reaction 1. The equilibrium position is the same in both the catalyzed reaction and the uncatalyzed reaction. The equilibrium position of the catalyzed reaction is shifted toward the products side. The equilibrium position of the catalyzed reaction is shifted toward the reactants side.
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)----> 2H2(g)+S2 kc= 1.67*10^-7 @ 800°C The reaction is carried out at the same temperature with the following initial concentrations: [H2S]= 4.50*10^-4 M [H2]= 0 M [S2]= 0 M Find the EQUILIBRIUM concentration of S2:
HOH₂C. HO CS NH₂ ·0 + لسلہ Glu H K₁f Kır HOH HO 0. HOH₂C CS-Glu + 2H₂O From what you know from Chapter 12 dealing with rate laws for an equilibrium reaction, derive Kc for the reaction above if we define Kc = k₁f/k₁r.
+ Imagine 212. mmol of HCH,CO, are removed from a flask containing a mixture of HCH,CO,, H,O, H,O' and CH,CO, at equilibrium, and then answer the following questions. Zero. What is the rate of the forward Greater than zero, but less than the rate of the reverse reaction. reaction before any HCH3CO2 has been removed from the flask? Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward Greater than zero, but less than the rate of the reverse reaction. reaction just after the HCH3CO2 has been removed from the flask? Greater than zero, and equal to the rate of the reverse reaction. Greater than zero, and greater than the rate of the reverse reaction. Zero. What is the rate of the forward Greater than zero, but less than the rate of the reverse reaction. reaction when the system has again reached equilibrium? Greater than zero, and equal to the rate of the reverse…
Please don't provide handwriting solution
part b please
*** S 19. Solid ammonium hydrogen sulfide is introduced into a 2.00-L flask, and the flask is şealed. If this solid decomposes according to the equation below DAUS Ca Nothange NH4HS(s) NH3(g) + H₂S(g), Kp = 0.108 at 25°C, what is the minimum mass of ammonium hydrogen sulfide that must be present in the flask initially if equilibrium is to be established at 25°C? A) 0.917 g B) 1.37 g C) 2.74 g D) 0.581 g E) 0.452 g
Predicting relative forward and reverse rates of reaction in a dynamic... Nitrogen and hydrogen react to form ammonia, like this: N2(g)+3H2(g) — 2 NH3(g) Imagine 61. mmol of NH3 are added to an empty flask, and then answer the following questions. What is the rate of the reverse reaction before any NH3 has been added to the flask? What is the rate of the reverse reaction just after the NH3 has been added to the flask? What is the rate of the reverse reaction at equilibrium? How much NH3 is in the flask at equilibrium? Zero. Greater than zero, but less than the rate of the forward reaction. Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and greater than the rate of the forward reaction. Zero. Greater than zero, but less than the rate of the forward reaction. Greater than zero, and equal to the rate of the forward reaction. Greater than zero, and greater than the rate of the forward reaction. Zero. Greater than zero, but less than the rate of the…