13. K. for the decomposition of ammonium hydrogen sulnde is 1.8 x 10-4 at 25 °C. The reaction. NH4HS(s) NH3(g) + H2S(g) a When the pure salt decomposes in a flask, what are the equilibrium concentrations of NH3 and H2S? b. If NH4HS is placed in a flask already containing 0.020 M of NH3 and then the system is allowed to come to equilibrium, what are the equilibrium concentrations of NH3 and H2S?

13. K. for the decomposition of ammonium hydrogen sulnde is 1.8 x 10-4 at 25 °C. The reaction. NH4HS(s) NH3(g) + H2S(g) a When the pure salt decomposes in a flask, what are the equilibrium concentrations of NH3 and H2S? b. If NH4HS is placed in a flask already containing 0.020 M of NH3 and then the system is allowed to come to equilibrium, what are the equilibrium concentrations of NH3 and H2S?

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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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
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4. Initially, a mixture of o.200 M NO, o.100 M Hs, O.200 M H.O was permitted to reach equilibrium (initially there was no Na). At equilibrium, the concentration of NO was discovered to be o.o62 M. Determine the value of the equilibrium constant, Ke, for the reaction: 2 NO(g) + 2 H2(g) S N2(g)+2 H20(g)
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12. The following gases are added to a 1.00 L container: 2.0 mole of A; 4.0 mole of B. The gases react as follows: A (g) + 3B (g) = C (g) + 2D (g) a. Create an ICE table to indicate the initial concentrations, the change in concentrations with respect to x, and the equilibrium concentrations al all the reactants and produces with respect to x. b. If the container contains 0.4 moles of D at equilibrium, calculate the equilibrium concentrations of A, B, C, and D. c. Calculate the value for the equilibrium constant at this temperature.
Carbon monoxide may be reacted with hydrogen to yield solid carbon and water vapor according to the reaction below. When the contents of a 1.000L reaction vessel are at equilibrium the components have the following amounts: 14.5mol C, 12.9mol H₂O, 3.52mol CO, and 2.43mol H₂ H₂ and H₂O Calculate Ke What are the concentrations of CO the new equilibrium? CO +Huy… CHỌ at
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