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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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
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Consider the following reaction: HSO4-(aq)+H2)(l)<--> H3O+(aq)+SO42-(aq) Kc=0.012 The initial concentrations are [HSO4-]=0.50M, [H3O+]=0.020M, [SO42-]=0.060M. Which way would the reaction shift to reach equilibrium? What are the equilibrium concentrations of the products and reactants?
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:
3. Predict the shift in the following equilibrium system resulting from each of the following changes: 4 HCI (g) + O, (g) = 2 H,O(g) + 2 Cl, (g) + 113 kJ c. an increase in the concentration of oxygen d. the addition of a catalyst
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3. Dinitrogen tetroxide, N2O4, dissociates at room temperature to give nitrogen dioxide, NO2. N2O4 (g) = 2 NO2 (g) The equilibrium constant Kç at 25°C is 0,125. What percentage of dinitrogen tetroxide is dissociated when 0,0300 mol N204 is placed in a 1,00 dm3 flask and left to reach equilibrium? (а) (b) The amount of nitrogen dioxide formed increases as the temperature rises. Is the dissociation of N2O4 endothermic or exothermic?