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plz explain
![An alternative equilibrium that could be used to explain the conversion of tetrahedrally
coordinated Co²+ in 2-propanol to the octahedral from upon addition of methanol is represented
by the following:
[CoCIP3]+ + 5 M = [COCIM,]+ + 3 P
a. Write an equilibrium expression for Keq for this reaction.
Reaction 4
b. Use the following experimental data determined at 22°C, to determine Keq.
Beaker
A
[Cotet]
1.25 x 10-3
[Cooct]
2.50 x 10-4
[P]
[M]
11.8
2.47
B
8.05 x 104
6.95 x 104
11.1
3.70
C
6.87 x 104
8.13 x 104
10.5
4.94
C.
Keq
Based on your answers to (b), is this alternative equilibrium possible? Explain.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb293ed07-3341-4776-8286-734d37a0eb0b%2F8e448dec-9b99-4742-ab44-5463d588c486%2Fcdmti4n_processed.png&w=3840&q=75)
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- 7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.Predict and calculate the effect of concentration changes on an equilibrium system. Some (CH3)2CHOH is allowed to dissociate into (CH3)2CO and H₂ at 452 K. At equilibrium, [(CH3)2CHOH] = 0.294 and [(CH3)₂CO] = [H₂] = 5.94x10-2 M. Additional (CH3)2CO is added so that [(CH3)2CO]new = 9.02x10-2 M and the system is allowed to once again reach equilibrium. (CH3)2CHOH(g)(CH3)2CO(g) + H₂(9) (a) In which direction will the reaction proceed to reach equilibrium? (b) What are the new concentrations of reactants and products after the system reaches equilibrium? [(CH3)2CHOH] = [(CH3)2CO] = [H₂] M M M = 1.20x10-2 at 452 K23-For the system 2 SO2(g) + O2(g) →2 SO3(g) , AH is negative for the production of SO3. Assume that one has an equilibrium mixture of these substances. Predict the effect of each of the following changes on the value of the equilibrium constant and on the number of moles of SO3 present in the mixture at equilibrium. Briefly account for each of your predictions. (Assume that in each case all other factors remain constant.) (a) Decreasing the volume of the system. (b) Adding oxygen to the equilibrium mixture. (c) Raising the temperature of the system.
- Consider the reaction: CH3COOH (aq) + H₂O(1) K = 1.8 x 10-5 at 25 °C Part A If a solution initially contains 0.225 mol L-¹ CH3COOH, what is the equilibrium concentration of H3O+ at 25 °C? Express your answer in moles per litre to two significant figures. 15. ΑΣΦ [H3O+] = H3O+(aq) + CH3COO (aq) Submit Request Answer ? mol L-1Phosphorus pentachloride thermally dissociates according to reaction given below.PCl5(g) ⇌ PCl3(g) + Cl2(g)a) What is the equilibrium expression, in term of mole fractions, for this reaction?b) What is the mole fraction, Xi , in terms of α, for each species present? Here, α is the degree of dissociation of the reaction.c) If the degree of dissociation is 0.920 at 600 K and 5.0 bar, what is the value of the equilibrium constantConsider the reaction: C(s) + 1/2O₂(g) = CO(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: C(s) + O₂(g) → CO₂(g) K₁ CO(g) + 1/2O₂(g) = CO2 (9) K₂ For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K =
- Predict and calculate the effect of concentration changes on an equilibrium system. Some CH-CH₂OH is allowed to dissociate Into C&H CHO and H₂ at 523 K. At equilibrium, [C6H5CH₂OH] = 0.195 M, and [CH,CHO] [H₂] = 5.03x10-2 M. Additional C₂H-CH₂OH is added so that [CH-CH₂OH]new = 0.319 M and the system is allowed to once again reach equilibrium. CHCH₂OH(g) C₂H5CHO(g) + H₂(g) = (a) In which direction will the reaction proceed to reach equilibrium? [ (b) What are the new concentrations of reactants and products after the system reaches equilibrium? [CHCH₂OH]= [CHyCHO] [H₂] M K= 1.30x10 at 523 K M MConsider the reaction: C(s) + O₂(g) → CO₂(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, K₁ and K₂, for the reactions below: C(s) + 1/2O₂(g) = CO(g) K₁ CO(g) + 1/2O₂(g) = CO2 (9) K2 For answers with both a subscript and a superscript, enter the subscript first. For example, enter K if the first equilibrium constant should be squared. K=3. Answer all sections (i) - (iv). 1 mole of ethanol (C2H5OH) and 1 mole of ethanoic acid (CH;COOH) were reacted at 25 °C, in a non- aqueous solvent, until equilibrium was reached. It was subsequently determined that 0.33 moles of ethanol remained at equilibrium. (i) Write an equation for the reaction. (ii) Write an expression for the equilibrium constant, Kc, for the reaction and calculate its value. Subsequently a further 3 moles of C2H5OH was added to the solution. (ii) Determine the concentrations of all the species present when equilibrium is restored.
- Consider the following equilibrium reaction: 2 CH3OH + CH2O ⇌CH2(OCH3)2+ H2O ΔH = + 46 indicate the direction that the equilibrium will shift when the following changes are made.(No states are provided because the solvent for the reaction is not water, so aq for aqueous would not be appropriate.) (a)Concentration of CH3OH increases (b)H2O is removed from the reaction (c)Reaction is heatedQ1I. Define equilibrium constant of a reaction II. When one mole of pure ethanol is mixed with one mole of ethanoic acid at room temperature, the equilibrium mixture contains 2/3 of a mole each of the ethyl ethanoate and water. Calculate the equilibrium constant for the reactionThe reaction N2O4−⇀↽−2NO2 is allowed to reach equilibrium in a chloroform solution at 25 ∘C . The equilibrium concentrations are 0.327 mol/L N2O4 and 1.91 mol/L NO2 . Calculate the equilibrium constant, Kc , for this reaction. Kc= 11.16 An additional 1.00 mol NO2 is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the NO2 is added. towards the product towards the reactant no change Determine how the addition of extra NO2 in the previous step will affect the rate constant, Kc . Kc will increase Kc will not change Kc will decrease Calculate the equilibrium concentrations of N2O4 and NO2 after the extra 1.00 mol NO2 is added to 1.00 L of solution. [N2O4]= mol/L [NO2]= mol/L
