Use data in Table 2.1, calculate the equilibrium constant, Ke for reactionsa. 2S02 (g) + O2 (g) = 2S03 (g)b. 2S0s (g) 2SO2 (g) + O2 (g)7.Initial concentrations, M Equilibrium concentrations, M(SO.](02] (SO)(SO2](SO)Experiment(a)0.800 0.4000.6880.3160.112Experiment(b)0.800.5900.4410.113Table 2.1: An experimental results of initial and equilibrium concentrations for reaction of SO2with Oz and the dissociation of SO3.

A numerical problem based on Kc for dissociation and formation of SO3, which is to be accomplished.

Use data in Table 2.1, calculate the equilibrium constant, Ke for reactions a. 2s02 (g) + O2 (g) 2SO3 (g) b. 2S0 (g) 2sO: (g) + O2 (g) Initial concentrations, M Equilibrium concentrations, M (SO.) (0:) (SO.) (SO2) (0:) Experiment (a) 0.800 0.400 0.688 0.316 0.112 Experiment (b) 0.80 0.590 0.441 0.113 Table 2.1: An experimental results of initial and equilibrium concentrations for reaction of SO2 with Oz and the dissociation of SO.

Use data in Table 2.1, calculate the equilibrium constant, Ke for reactions a. 2s02 (g) + O2 (g) 2SO3 (g) b. 2S0 (g) 2sO: (g) + O2 (g) Initial concentrations, M Equilibrium concentrations, M (SO.) (0:) (SO.) (SO2) (0:) Experiment (a) 0.800 0.400 0.688 0.316 0.112 Experiment (b) 0.80 0.590 0.441 0.113 Table 2.1: An experimental results of initial and equilibrium concentrations for reaction of SO2 with Oz and the dissociation of SO.

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

Do
9 Methanol is produced synthetically: CO (g) + 2H2 (g) CH;OH (g) A H=+24 Kcal a) Write the Equilibrium Constant Expression: b) Is it an Endothermic or Exothermic Reaction? c). Indicate the effect on the equilibrium, ie., does the reaction shift to the right, to the left, or have no effect on the reaction at all: 1. Increase in [2H2] = 2. Decrease in [CO] = 3. Increase in Temperature = 4. Increasc in Pressure = 5. Addition of a catalyst =,
ACTIVITY 1: Let's Practice: In this activity answer some following problems and proof if the reaction is going forward or reverse. (On a Piece of Paper) Write the equilibrium constant expression, Kc, for the following reactions. А. Indicate also if the equilibrium is homogeneous or heterogeneous. A. 2 Ag(9) + Zntaa) = 2 Agčaa) + Zns) B. 2 C,H4c9) + 2 H20zc@) = C2H6(9) + 0zc@) C. Cs) + 2 HA@)= CH«@) D. 4 HCl(aq) + 0z(9) = 2 H201) + 2 Clz®)
Q2 For the chemical reaction shown below select the correct the equilibrium constant expression for 4NH3(g) + 302(g) = 2N2(9) + 6H2O(g) Q3 4NH3(9) + 302(9) = 2N2(9) + 6H2O(9) If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (02) gas in a 7.95 Liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas then how many moles of ammonia (NH3) is present at equilibrium? 4NH3(9) + 302(9) 2N2(9) + 6H2O(g) Q4 If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (02) gas in a 7.95 Liter air tight metal flask at 127°C and after the pressures stabilizes at equilibrium and then draws an air sample and found 0.683 moles of nitrogen (N2) gas then how many moles of water (H,O) is present at equilibrium? 4NH3(9) + 302(g) 2N2(9) + 6H2O(9) Q5 If a chemist mixed 2.930 moles of ammonia (NH3) gas with 1.978 moles of oxygen (02) gas in a 7.95 Liter air…
for equilibrium 2SO2 + O2 = 2SO3 for a certain temperature has Ke = 1.06 What effect would it have on the value of the constant: a) lowering the temperature b) use of the catalyst c) increase of SO2 concentration 2. Explain the effect of the factors presented above for the system in equilibrium: a) with decreasing temperature b) with the use of a catalyst c) with increasing SO2 concentration
Carbon monoxide can form carbon dioxide via the reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.19 mol of CO remaining. Keq at the temperature of the experiment is __________. A) 1.78 B) 0.75 C) 0.56 D) 5.47 E) 1.0
Find equilibrium concentration of this product? Dont 100% know how to manipulate ICE chart to solve this. Thanks
Image uploaded answer is not allowed please dear expert.
The following reaction is at equilibrium: N2{g) + 3H2(g)22NH3(g) The equilibrium concentration for N2 and H2 are 0.22 M and 0.4 M, respectively. If the Keq is 0.78, what is the equilibrium concentration of NH3? Enter your answer using 3 decimal places and without unit.
Identify the correct equilibrium constant expression for the reaction: Nz (9) + ЗH2 (g) < — 2NH3 (9) [N2][H2]³ [NH3]? K : [2NH3] К — K [N2][3H2] [NH3]? [N2][H2]³ K [2NH3]? [N2][3H2]3 K = %3D
Open the photo
Chapter 12 part 3