DH M000101o Jm00 2S tivw baxim cHM MO00S.0 to Jnt02.SS 19. Solid NH4HS decomposes by the following endothermic reaction: NH4HS(s) b NH3(g) H2S(g) Jm00.es a. What effect would adding more NH3 have on the equilibrium? b. What effect would adding more NH4HS have on the equilibrium? c. What effect would increasing the volume of the container have on the equilibrium? d. What effect would decreasing the temperature have on the equilibrium?

DH M000101o Jm00 2S tivw baxim cHM MO00S.0 to Jnt02.SS 19. Solid NH4HS decomposes by the following endothermic reaction: NH4HS(s) b NH3(g) H2S(g) Jm00.es a. What effect would adding more NH3 have on the equilibrium? b. What effect would adding more NH4HS have on the equilibrium? c. What effect would increasing the volume of the container have on the equilibrium? d. What effect would decreasing the temperature have on the equilibrium?

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...

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d. he following system establishes an equilibrium at 545 K: NH₂HS (s)- NH₂ (8) + H₂S (8) AND >O Briefly explain the effect in terms of the expected shift (toward reactant, toward product or no change) of each of the following: a b. The volume of the container is doubled. The temperature of the system is raised to 825 K C. Some additional solid NH4HS is added. The reaction flask has 1.25 atm of the inert gas argon added to it. 5. (10 points) At 355 K, a 10.00 L reaction flask is charged with 1.44 atm each of hydrogen and fluorine gas. The following reaction takes place: H2 (8) + F2 (g) = 2 HF (g) Kp = 176 Based on building an ICE table, determine the partial pressure of H2, F2 and HF once equilibrium has been established.
Calculate the Keq from the given concentrations, all are gases. start: equilibrium: Kegf= C₂H6 + 1.000 M 0.750 M k. HS-1 2 Cl₂ 1.000 M 0.500 M 0.500 M used Keof= a. H30+1 b. OH-1 c. C₂H6 j. H₂S u. 8.00 x 10-5 1. S-² v. 1.75 x 10-6 bb. 0.6000 cc. 1.104 x 10-5 5 First put in the chemicals, then put in the numbers. The concentrations for both Cl₂ and HCI are squared due to their coefficients. ][ 1² |² ][ C₂H4Cl₂ + 0.000 M 0.250 M 2 HCI 0.000 M 0.500 M 1² ( d. C₂H4Cl₂ e. Cl₂ o. 0.750 m. HX n. X-1 w. 1.11 x 108 x. 5.5 x 10-2 dd. 0.7100 ee. 1.26 x 10-5 f. HCI g. H₂SO3 q. 1 p. 2 y. 0.7000 ff. 4.901 X h. HC2H3O2 i. C₂H30₂-¹ s. 0.500 t. 0.333 aa. 1.143 x 105 hh. 4.942 ii. 4.957 r. 0.250 z. 1.60 x 10-5 gg. 7.93 ²
COVID-19 & Health e. Kc = [NH3]² · [CO2] For which reactions will the position of equilibrium shift due to changing the volume of the container. Select one: O a. Only reactions which have more gaseous products than reactants. O b. Only reactions where the number of moles of gas changes. c. All reactions involving a gas. d. All reactions where the number of moles change. O e. Only reactions which have less gaseous products than reactants. Select the correct cell notation for the following reaction, which is setup as a cell with a platinum electrode:
Write the equilibrium expressions for the following given reactions. a. Br2 + 2HI --------------> I2 + 2HBr b. 2NaHCO3(s) --------------------> Na2CO3(s) + CO2(g) + H2O(g) 1. Bromine monochloride (BrCl) decomposes to form bromine and chlorine: 2BrCl(g) -------> Br2(g) + Cl2(g) At a certain temperature, the equilibrium constant for the reaction is 11.1. A sample of pure BrCl is placed in a 1.0 L container and allowed to decompose. At equilibrium, the reaction mixture contains 4.0 mol Cl2. What are the equilibrium concentrations of Br2 and BrCl? 2. Iodine molecules react reversibly with iodide ions to produce triiodide ions. I2(aq) + I-(aq) ----------> I3(aq) If a liter of solution prepared from 1.00x10-3 mol of I2 and 1.00x10-3 mol of the strong KI contains 6.61x10-4 mol of iodine at eq., what is the eq. constant for the reaction? Establish an ICE chart.