Gaseous hydrogen iodide is placed in a closed 5.00-L container at 458°C, where it partially decomposed to hydrogen and iodine: 2HI(g) = H2(g) + 12(g). At equilibrium, it is found that [H2] = 2.24x10-2 M, [12] = 2.24x10- 2 M and [HI] = 0.155 M. What are the equilibrium concentrations when equilibrium is reestablished following the addition of 0.100 mol if HI?

Gaseous hydrogen iodide is placed in a closed 5.00-L container at 458°C, where it partially decomposed to hydrogen and iodine: 2HI(g) = H2(g) + 12(g). At equilibrium, it is found that [H2] = 2.24x10-2 M, [12] = 2.24x10- 2 M and [HI] = 0.155 M. What are the equilibrium concentrations when equilibrium is reestablished following the addition of 0.100 mol if HI?

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

The equilibrium system 2A <-> 2B + C has a very small equilibrium constant: K = 2.6 ´ 10–6. Initially 3.0 moles of A are placed in a 1.5-L flask. Determine the concentration of C at equilibrium.
please explain and give complete answer
For the reaction N,0,(g) = 2NO,(g) Kc = 4.66 × 10-3 at 25°C . 2.50 g N,04 and 0.190 g NO, are introduced into a 2.00-L reaction vessel. After equilibrium is achieved, what is the concentration of NO,?
The equilibrium constant, K, for the following reaction is 2.90×10-2 at 1.15×10³K. 2S03(g) 2S02(g) + 02(g) If an equilibrium mixture of the three gases in a 14.5 L container at 1.15×10³K contains 0.367 mol of SO3(g) and 0.356 mol of SO2, the equilibrium concentration of O, is M.
The equilibrium constant, Ko, for the following reaction is 1.80x104 at 298 K. NH4HS(s) =NH3(g) + H2S(g) Calculate the equilibrium concentration of H2S when 0.428 moles of NH4HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S]
The equilibrium constant for the reaction NO3 (g) + NO (g) «> 2NO2, (g) is 0.76 at 150°C. If 0.800 mol of NO, was reacted with 0.800 mol of NO in a 1.25 L closed container, what will be the equilibrium concentration of NO2?
The equilibrium constant, Kc , for the following reaction is 0.0290 at 1150 K. 2SO3= 2SO2 + O2 If an equilibrium mixture of the three gases in a 17.7 L container at 1150 K contains 0.316 mol of SO3 and 0.452 mol of SO2, the equilibrium concentration of O2 is M.
Hydrogen iodide decomposes according to the reaction 2HI(g) = H₂(g) + 1₂ (g) A sealed 1.50-L container initially holds 0.00623 mol of H₂, 0.00414 mol of 1₂, and 0.0244 mol of HI at 703 K. When equilibrium is reached, the concentration of H₂(g) is 0.00524 M. What are the equilibrium concentrations of HI (g) and I₂ (g)? Round each of your answers to 3 significant figures. Part 1 of 2 [HI] = M Part 2 of 2 [¹2]eq = M x10 x10 X x Ś S
The equilibrium constant, K, for the following reaction is 1.20x10-2 at 500K. PCI5(g) PCI3(g) + Cl2(g) If an equilibrium mixture of the three gases in a 15.3 L container at 500K contains 0.359 mol of PCI5(g) and 0.228 mol of PC13, the equilibrium concentration of Cl2 is М.
A student ran the following reaction in the laboratory at 1171 K: 2502(g) + O₂(g) = 2503(9) When she introduced 7.80 x 10-2 moles of SO₂(g) and 8.76x102 moles of O₂(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(9) to be 4.35x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = Submit Answer Try Another Version 10 item attempts remaining
A student ran the following reaction in the laboratory at 709 K: N2g) + 3H2(g)2NH3(g) When she introduced 4.04x102 moles of N(g) and 6.09x102 moles of H2ig) into a 1.00 liter container, she found the equilibrium concentration of H2lg) to be 5.89x102 M. Calculate the equilibrium constant, K. she obtained for this reaction. K =
The equilibrium constant, Ke, for the following reaction is 10.5 at 350 K. 2CH,Cl(g) CH(g) + CCl(g) Calculate the equilibrium concentrations of reactant and products when 0.392 moles of CH,Cl, are introduced into a 1.00 L vessel at 350 K. [CH,Cl,] = M [CH4] M [CC4] M