Consider the following reaction where Kc = 10.5 at 350 K: 2 CH₂Cl₂ (9) CH4 (9) + CCI4 (9) A reaction mixture was found to contain 1.15x10-2 moles of CH₂Cl₂ (9), 5.27x10-2 moles of CH4 (9), and 3.67x10-2 moles of CCl4 (9), in a 1.00 liter container. Indicate True (I) or False (F) for each of the following: 1. In order to reach equilibrium CH₂Cl₂(g) must be consumed. 2. In order to reach equilibrium K must decrease 3. In order to reach equilibrium CH4 must be consumed. 4. Qc is less than Ke 5. The reaction is at equilibrium. No further reaction will occur.

Consider the following reaction where Kc = 10.5 at 350 K: 2 CH₂Cl₂ (9) CH4 (9) + CCI4 (9) A reaction mixture was found to contain 1.15x10-2 moles of CH₂Cl₂ (9), 5.27x10-2 moles of CH4 (9), and 3.67x10-2 moles of CCl4 (9), in a 1.00 liter container. Indicate True (I) or False (F) for each of the following: 1. In order to reach equilibrium CH₂Cl₂(g) must be consumed. 2. In order to reach equilibrium K must decrease 3. In order to reach equilibrium CH4 must be consumed. 4. Qc is less than Ke 5. The reaction is at equilibrium. No further reaction will occur.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 12E: Show that the complete chemical equation, the total ionic equation, and the net ionic equation for...

See similar textbooks

Similar questions

Consider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. â€¢ The density of the solution is 1.00 g/mL. â€¢ Volumes are additive. â€¢ The specific heat of the solution is 4.18 J/g C.
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
Write the expression for Keq for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous. H2(g) + I2(g) 2 HI(g) Keq = 2 PHI / (PH2 PI2) Keq = PH2 PI2 / 2 PHI Keq = PH2 PI2 / PHI2 Keq = PHI2 / (PH2 PI2)
Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C.
Calcium hydroxide is a base that does not dissolve very well in water. When saturated, a calcium hydroxide solution at 25°C contains 1,3 gram Ca(OH)2 per dm3 solution. The molar mass of Ca(OH)2 is 74,1 g×mol–1. When the Ca(OH)2 dissolves, the following reaction represents the solubility equilibrium: Ca(OH)2 (s) D Ca2+ (aq) + 2 OH– (aq) Use this information above to find the value of Ksp for Ca(OH)2 at 25°C. What is the pH of this saturated Ca(OH)2 solution?
Calculate the KC for the reaction N2 (g) + 3H2 (g) ⇌ 2NH3 (g) at 773.15 K if the KP = 1.5 x 10 - 5 at this temperature.
2.) For the reaction I2(g) ⇌ 2I(g), Kc = 3.8 x 10–5 at 727°C. (a) What is Kc for the reverse reaction at this temperature? (b) Calculate Kc for the reaction ½I2(g) ⇌ I(g).
3. Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g),SO2Cl2(g)⇌SO2(g)+Cl2(g), Kp Kp=2.91×103 at 298 KK In a reaction at equilibrium, the partial pressure of SO2SO2 is 0.135 torr and that of Cl2Cl2 is 0.370 torr. a. What is the partial pressure of CO2CL2 in this mixture? Express your answer in torr using three significant figures.
For the following reactionC(??) + 2H2(??) ⇌ CH4(??)K =0.26 at 1000 °C (3 significant figures). What is the equilibrium constant at 750 °C (3significant figures)?
a. For the reaction 2A(g)+2B(g)⇌C(g)2A(g)+2B(g)⇌C(g) Kc = 54.4 at a temperature of 71 ∘C . Calculate the value of Kp. Express your answer numerically. b. For the reaction X(g)+3Y(g)⇌2Z(g)X(g)+3Y(g)⇌2Z(g) Kp = 3.74×10−2 at a temperature of 117 ∘C . Calculate the value of Kc. Express your answer numerically.
Consider the following reaction where Kc = 77.5 at 600 K.CO(g) + Cl2(g) COCl2(g)A reaction mixture was found to contain 4.68×10-2 moles of CO(g), 4.17×10-2 moles of Cl2(g) and 0.123 moles of COCl2(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals .The reactionfill in the blank 2A. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.
Calculate the numerical value of the Kp for: N2(g) + 3H2(g) ⇌2NH3(g) Kc=5.8x105 at 25°C. A. 9.7x102 B. 5.8x105 C. 3.5x108 D. 3.6x1012