Review Constants Period Part A A mixture initially contains A, B, and C in the following concentrations: A 0.650 M, B = 0.800 M, and [C] = 0.600 M. The following reaction occurs and equilibrium is established: A + 2B C At equilibrium, [A = 0.460 Mand [C] = 0.790M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically. > View Available Hint(s) VO AE¢ ΑΣΦ K. = Submit 7:43 PM /13/2020 hp

Review Constants Period Part A A mixture initially contains A, B, and C in the following concentrations: A 0.650 M, B = 0.800 M, and [C] = 0.600 M. The following reaction occurs and equilibrium is established: A + 2B C At equilibrium, [A = 0.460 Mand [C] = 0.790M. Calculate the value of the equilibrium constant, Ke. Express your answer numerically. > View Available Hint(s) VO AE¢ ΑΣΦ K. = Submit 7:43 PM /13/2020 hp

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...

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2 Name: Maile Velazquez Date: Period: 6 H-02 Equilibrium Assignment Instructions: Write the Law of Mass Action for each of the following chemical equations and then calculate the indicated missing variable using the provided information while at equilibrium. Ex H2O + COH₂+ CO₂ 1H2O+ 1CO1H2 + 1CO₂ [H2]¹[CO2]¹ K₂ = Кс 4.73 [H,O][CO] [CO2] = [H2]¹ (4.73)(0.0322)(0.0510) [H2O] 0.0322 M [CO₂] = = 0.0135088 (0.575) [CO] 0.0510 M [H2]¹[CO2] [CO2] = 0.0135 M [H2] 0.575 M [H,O][CO] H₂+2 A₁₂+ B₂ → AB3 [AB3] 0.146 M [A₂] 1.50 M K = K₁ = [B2] 0.240 M
Consider the reaction of SO2 and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. NEXT > A 2.00 L reaction vessel was filled 0.0432 mol SO2 and 0.0296 mol O2 at 900 K and allowed to react. At equilibrium, the concentration of SO3 was found to be 0.0175 M. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.00875 0.0209 0 0.00875 2 SO₂(g) + O₂(g) = 2 SO³(g) 2SO2(g) 2.00 0.0216 0.0432 0.0148 + 0.0296 0.0041 O₂(g) 2 0.0175 0.0129 -0.0175 0.0061 2SO3(g) RESET -0.0350 0.0257
Question 2, part c: please see attached Part a answer: if an initial concentration before equilibrium of c2h4o2 is 0.080 M, what are the equilibrium conc of the three species in the equilibrium: [H3O+]=[C2H3O2-]=1.20x10^-3M Part b answer: a solution in which this reaction takes place is analyzed and found to have [C2H4O2]=0.073M and [C2H3O2-]=0.251M and pH 2.131. Is the system and equilibrium? Calculate Q Qc=2543.0 x 10^-5 Kc=1.81 x 10^-5 not at equilibrium
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0.050 M of H2 and 0.050 M of Brz are placed in an evacuated 5.0 L flask and heated to 700 K. What is the concentration of HBr in the flask when equilibrium has been established? The equation for the reaction is as follows: H2(g) + Br2(g) = 2HBr(g) K= 64 @ 700 K Round your answer to 3 decimal places.
Question 3
ⒸMacmillan Learning Write the chemical reaction for chlorous acid in water, whose equilibrium constant is K₂. Include the physical states for each species. K₁ reaction: HCIO, (aq) + H₂O(aq) → H₂O¹(aq) + C1O₂ (aq) = Write the chemical reaction for the chlorite ion in water, whose equilibrium constant is K. Include the physical states for each species. Kreaction: CIO₂ (aq) + H₂O(aq) ⇒ HC10₂(aq) + OH¯(aq)|
Answer only no. 2, increased temperature and increased pressure
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