At 500 °C, hydrogen iodide decomposes according to2 HI(g) = H, (g) + I,(g)For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium:[H,] = 0.300 M, [I,] = 0.300 M, and [HI] = 2.54 M. If an additional 1.00 mol of HI(g) is introduced into the reactionvessel, what are the equilibrium concentrations after the new equilibrium has been reached?[HI] =M[H] =M[L] =M

Solution : A decomposition reaction is when a compound is broken down into two or more…

At 500 °C, hydrogen iodide decomposes according to 2 HI(g) = H,(g) + I,(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H,] = 0.300 M, [L,] = 0.300 M, and [HI] = 2.54 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI] [H.] = L] =

At 500 °C, hydrogen iodide decomposes according to 2 HI(g) = H,(g) + I,(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H,] = 0.300 M, [L,] = 0.300 M, and [HI] = 2.54 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI] [H.] = L] =

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

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,?
For the reaction 2SO2(g) + O2(g) ⟺ 2SO3(g) at a certain temperature, the equilibrium concentrations were observed to be [SO2] = 0.646 M, [O2] = 7.50 × 10–2 M, and [SO3] = 0.650 M. Calculate the value of K for this system at this temperature.
For the reaction 3 A --> B + 2C, 3.60 mol A is placed in a 3.00 L vessel. At equilibrium the concentration of B is 0.300 M. Determine the value of the equilibrium constant, Kc.
A student ran the following reaction in the laboratory at 288 K: 2NO(g) + Br2(g) = 2NOBr(g) When she introduced 0.140 moles of NO(g) and 0.117 moles of Br,(g) into a 1.00 liter container, she found the equilibrium concentration of NOBR(g) to be 0.108 M. Calculate the equilibrium constant, K., she obtained for this reaction. K. =
A student ran the following reaction in the laboratory at 1152 K: 2502(g) + 02(g) = 2503(g) When she introduced 7.99x102 moles of so, (g) and 7.30x102 moles of 02(g) into a 1.00 liter container, she found the equilibrium concentration of SO3(g) to be 4.51×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K =
Explain step by step
A mixture initially contains A, B, and C in the following concentrations: [A] = 0.700 M, B] = 0.950 M , and [C = 0.500 M. The following reaction occurs and equilibrium is established: A + 2B = C At equilibrium, [A] = 0.510 Mand C = 0.690 M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically.
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 1152 K: 2502(g) + 02(g) = 2s03(g) When she introduced 7.99x102 moles of So2(g) and 7.30x10 2 moles of 02(g) into a 1.00 liter container, she found the equilibrium concentration of So3 (g) to be 4.51×10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. K. =
A student ran the following reaction in the laboratory at 543 K: CoCl₂(g) CO(g) + Cl₂(g) When she introduced 1.10 moles of COCI₂(g) into a 1.00 liter container, she found the equilibrium concentration of Cl₂(g) to be 3.94-102 M. Calculate the equilibrium constant, K, she obtained for this reaction.
A student ran the following reaction in the laboratory at 279 K: 2CH,Cl,(g)CHĄ(g) + CC14(g) When she introduced 8.03x102 moles of CH,Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of CCl(g) to be 3.76x102 M. Calculate the equilibrium constant, K, she obtained for this reaction. K =|
At a certain temperature, the equilibrium constant, K., is 0.00572 for the reaction Cl,(g) = 2 Cl(g) A. If 2.77 g Cl, is placed in a 2.50 L flask at this temperature, what are the equilibrium concentrations of Cl, and Cl? [CI,] = M [CI] = M B. Following the establishment of equilibrium in part A, the volume of the flask is suddenly increased to 5.00 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and Cl? [Cl,] = M [CI] = M C. Following the establishment of equilibrium in part A, the volume of the flask is instead suddenly decreased to 1.0 L while the temperature is held constant. What are the new equilibrium concentrations of Cl, and CI? [Cl,] = M [CI] = M