The equilibrium constant, K., for the following reaction is 1.80×10 at 298 K. NH,HS(s) NH3(g) + H,S(g) If an equilibrium mixture of the three compounds in a 4.38 L container at 298 K contains 2.09 mol of NH,HS(s) and 0.241 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 8 more group attempts remaining

The equilibrium constant, K., for the following reaction is 1.80×10 at 298 K. NH,HS(s) NH3(g) + H,S(g) If an equilibrium mixture of the three compounds in a 4.38 L container at 298 K contains 2.09 mol of NH,HS(s) and 0.241 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 8 more group attempts remaining

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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(a) Determine whether the value of K of an equilibrium system will be affected or, unaffected by the following changes: Changes Value of K (affected or unaffected) (O Decreasing the temperature (1) Increasing the pressure of the system () Decreasing the concentration of reactant (b) The following graph represents the amount of CO formed at two different temperatures, T; and T. The reaction as shown below: C() + H,O(g) = co(g) + H(g) T = 385 K [co) T = 335 K time Based on the graph, determine whether the forward reaction is endothermic or exothermic. Predict if the concentration of H:0 gas increases, decreases or remains the same if the temperature is decreased to 298 K. Explain. A mixture of 0.350 M of H:0, 0.125 M of CO and 0.125 M of H: was prepared and allowed to reach equilibrium in a 1.00 L flask. The equilibrium concentration of H;0 is 0.182 M. Calculate the Ke of the reaction at constant temperature. (H)