10) Describe the effect of each stress below on the following equilibrium in a closed vessel. NH3 (g) + H2S (g) 5 NH,HS (s) (exothermic) Effect on Effect on Effect on Direction of Forward Rate Reverse Rate Effect on Q Effect on Kc amount of H2S Shift of Reaction of Reaction Remove H2S Remove NH&HS Add NH3 Triple the Volume Be quantitative Warm up Grind up the NH4S

10) Describe the effect of each stress below on the following equilibrium in a closed vessel. NH3 (g) + H2S (g) 5 NH,HS (s) (exothermic) Effect on Effect on Effect on Direction of Forward Rate Reverse Rate Effect on Q Effect on Kc amount of H2S Shift of Reaction of Reaction Remove H2S Remove NH&HS Add NH3 Triple the Volume Be quantitative Warm up Grind up the NH4S

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

please jdhjdjdodjbdnkxkx
Heleppppelppppppppp
There are two parts to this question. Each part is attached in separate pictures.
For the reaction Br2(g) + Cl2(g) 2BrCl(g), at equilibrium, it is found that the concentrations of Br2, C12, and BrCl are 0.484 M, 0.105 M, and 1.24 × 10 M, respectively. What is the value of Kc? 3 3.01 × 10-5 3.32 x 104 2:43 × 10-2 1.20 × 10-4
Give typed solution
Part B please
Which of these situations will result if some CH4lg) Is removed from the reaction Colg) + 3H2(g) = CH4(9) + H20(g) at equilibrium? Multiple Choice More CHa and H2O will be produced. No change will occur. Ko Will decrease. More CO will be produced. H20 will be consumed.
c hddjkfxkkc please
0.400 + x Predict the equilibrium concentration of IBr in the reaction described below (for which Kc = 280 at the reaction temperature) by constructing an ICE table, writing an equilibrium expression for Kc, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. ₂(g) + Br₂(g) 2 lBr(g) NEXT > In a 3.0 L container at high temperature, 0.400 mol of IBr is allowed to reach equilibrium. Fill in the ICE table with the appropriate value for each involved species to determine the partial pressures of all reactants and products. Where applicable, use the x variables to represent any unknown change in concentration. Initial (M) Change (M) Equilibrium (M) 0 0.400 + 2x 1 0.400 0.400- x 1₂(g) 0.133 0.400 - 2x 2 + Br₂(g) = +x 3 0.133 + x +2x 0.133 + 2x 2 IBr(g) -X 0.133 - x ORESET -2x 0.133 - 2x
14. The following reaction is allowed to come to equilibrium and then the volume is increased. Predict the effect of the indicated volume change once equilibrium is restored. H2O(g) + CO2(g) double arrow H2CO3(g) The reaction will shift right. The reaction will shift left. There will be no effect. Effect can not be determined from information provided.
Choose the correct equilibrium constant expression corresponding to Kc for the heterogeneous reaction O O Ke о Kc = OKc 2 [H₂01² [0₂][CH4] Kc = Ke 2[H₂O]² [0₂] [CH4] = Ke [02₁] 1 [0₂][CH₁] [H₂O]2[C] [0₂][CH4] CH4(g) + O₂(g) = C(s) + 2H₂O(g)
Problem-Solving Strategies: Understanding Equilibrium ▼ Part A Identify the stress Consider the equilibrium reaction CO(g) + H₂O(g) - CO₂(g) + H₂(g) Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response. Drag the appropriate labels to their respective targets. ► View Available Hint(s) Increase reactant Decrease reactant Increase product Decrease product Submit Type here to search Reverse reaction rate temporarily increases Forward reaction rate temporarily increases Forward reaction rate temporarily decreases Reverse reaction rate temporarily decreases Change Add CO(g) Remove H₂O(g) Add CO₂(g) Remove H₂(g) I H System stress Group 1 Group 1 Group 1 Group 1 ✔ Ca Equilibrium shift Group 2 Group 2 Group 2 Group 2 Reset Help