The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. NH4HS(9) NH3(g) + H₂S(g) Calculate the equilibrium concentration of H₂S when 0.322 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H₂S] = M Submit Answer Retry Entire Group 9 more group attempts remaining ТОГ

The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. NH4HS(9) NH3(g) + H₂S(g) Calculate the equilibrium concentration of H₂S when 0.322 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H₂S] = M Submit Answer Retry Entire Group 9 more group attempts remaining ТОГ

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

Determine the value of Ke for the following reaction if the equilibrium concentrations are as follows: [P4010leq = 3.000 moles, [P4leq= 4.000 moles, [O2leg = 5.000 M %3D %3D %3D P4010(s) P4(6) +5 02(8) Select one: O a. 4.000 O b. 5.000 O C. 4167 O d. 12500 O e. 3125
The equilibrium constant, Kc, for the following reaction is 0.0180 at 698 K. 2HI(g) → H₂(g) + 12 (9) Calculate the equilibrium concentrations of reactant and products when 0.305 moles of HI(g) are introduced into a 1.00 L vessel at 698 K. HI [H₂] [1₂] = = = M 3 M
help me asap pls i'll give you upvote later for number 4
help me asap pls i'll give you upvote later for number 4
no need for solution answer onnly pleaseeee , im in a rush
At a certain temperature, Kc = 1.00 102 for the reaction given below. H2(g) + F2(g) equilibrium reaction arrow 2 HF(g) (a) Calculate the concentrations of all species in the equilibrium mixture produced by adding 3.10 mol of H2 and 3.10 mol of F2 to a 1.00 L container. H2 F2 HF (b) What would the equilibrium concentration of HF be if 1.50 mol of HF is removed from the equilibrium mixture in Part a?
Predict the equilibrium partial pressure of HBr in the reaction described below by constructing an equilibrium expression for Qp, constructing an ICE table, writing the equilibrium constant expression, writing an equilibrium expression for Kp expressed in partial pressures, and solving for the equilibrium partial pressure of HBr. Complete Parts 1-4 before submitting your answer. 2 HBr(g) = H₂(g) + Br₂(g) 2 3 NEXT > An initial mixture of 0.20 atm HBr, 0.010 atm H2, and 0.010 atm Br₂ reacts. Set up the expression for Qp to determine the direction of the reaction. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qp. (0.20) 5.0 x 10-4 (0.010) 0.050 1 Qp = 2(0.20) 0.0025 2(0.010) 2.0 × 10³ (0.20)² 4.0 x 10² = (0.010)² 4 2(0.20)² RESET 2(0.010)² +
What is the value of the equilibrium constant Ko for the following reaction at the temperature of the mixture? 2NO,(g) N,0,(g) 3rd attempt See Periodic Table O See Hint Analyses of an equilibrium mixture of N204(g) and NO2(g) gave the following results: [NO2(g)] = 4.210×10-3 M [N204(g)] = 2.706×10³ M 221.3
Iodine and bromine react to give iodine monobromide, IBr. I1 (9) + Brz (9) = 2IB:(9) What is the equilibrium composition of a mixture at 154°C that initially contained 1.10 x 10- mol each of iodine and bromine in a 5.00 L vessel? The equilibrium constant K, for this reaction at 154°C is 130. [1:] =( M [Bra] =( M [IBr] = M
1) Consider the reaction A3+(aq) + B-(aq) ⇌ AB2+(aq) A) In 1.00 Liter of water at equilibrium, there are 1.00 moles of A3+, 4.00 moles of B- and 8.00 moles of AB2+(aq). What is the value for the equilibrium constant?B) Draw an image to represent this initial state. (below)C) At some time, t, 13.00 moles of ABCl2 is added, the volume change is negligible. ABCl2 is acompletely soluble compound that forms AB2+(aq) and 2 Cl-(aq) ions, the chloride ions are spectatorions and do not affect the equilibrium, you do not have to include them in the diagram. Draw twomodels to represent this occurrence; one for the instant the substance was added and once to showthe reaction reestablishing the equilibrium.
The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. NH4HS (8) NH3(g) + H₂S(9) Calculate the equilibrium concentration of H₂S when 0.416 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H₂S] = M
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 × 10-4 at a certain temperature. If a solid sample of CaCro4 dissolves in solution, what will the equilibrium concentration of Ca2+ in the solution be? СаCrOa(s) — Cа" (аq) + CrO,7 (aq) 1 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. CaCrO4(s) Ca2*(aq) Cro,2 (aq) + Initial (M) Change (M) Equilibrium (M)