Concept explainers
a)
Interpretation:
Using the pKa values the direction in which equilibrium is favored in the reaction given is to be stated.
Concept introduction:
The direction in which equilibrium is favored in the reaction can be ascertained from the pKa values of the substances involved. Lower the pKa value, stronger the acid. Further the relative stabilization by resonance of the conjugate bases produced also has to be considered.
To determine:
The direction in which equilibrium is favored in the reaction using the pKa values given.
b)
Interpretation:
Using the pKa values the direction in which equilibrium is favored in the reaction given is to be stated.
Concept introduction:
The direction in which equilibrium is favored in the reaction can be ascertained from the pKa values of the substances involved. Lower the pKa value, stronger the acid. Further the relative stabilization by resonance of the conjugate bases produced also has to be considered.
To determine:
The direction in which equilibrium is favored in the reaction using the pKa values.
c)
Interpretation:
Using the pKa values the direction in which equilibrium is favored in the reaction given is to be stated.
Concept introduction:
The direction in which equilibrium is favored in the reaction can be ascertained from the pKa values of the substances involved. Lower the pKa value, stronger the acid. Further the relative stabilization by resonance of the conjugate bases produced also has to be considered.
To determine:
The direction in which equilibrium is favored in the reaction using the pKa values.
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Chapter 2 Solutions
ORGANIC CHEMISTRY-EBOOK>I<
- Illustrate the process of determining the direction of equilibrium using pKa ?arrow_forwardThe reaction of bromine gas with chlorine gas, shown below, has a Kc of 7.20 at 200 oC. If a closed vessel was charged with the two reactants, each at an initial concentration of 0.50 M, what would be the equilibrium concentration of Cl2(g)?arrow_forwardWhat is the equilibrium concentration (in M to three decimal places) of NO2 for the following reaction if the initial concentration of N2O4 was 0.250 M?arrow_forward
- During the day, solar radiation is absorbed by NO3(g)NO3(g), resulting in its decomposition. Which of the following best explains whether the equilibrium concentration of N2O5(g)N2O5(g) in the atmosphere in the daytime is different from that in the nighttime, and why?arrow_forwardA 1.00 L flask was filled with 2.00 mol gaseous SO2 and 2.00 mol gaseous NO2 and heated. After equilibrium was reached, it was found that 1.30 mol of gaseous NO was present. Assume that the reaction SO2(g) + NO2(g) SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reactionarrow_forwardThe equilibrium constant, Kc , for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) is 6.90 x 103 . (a) What is Kc for the reaction 2 SO3 (g) → 2 SO2 (g) + O2 (g) (b) What is Kc for the reaction SO2 (g) + 1/2 O2 (g) → SO3 (g)arrow_forward
- Most reaction do not go to completions. Equilibrium is established between the reactants and products. For the reaction of A with B to produce C and D, we can write the chemical equation as: аА + bв + сс + dD where + represents equilibrium between the reactants and products. The extent to which the reaction proceeds to product formation, at a given temperature, is given by the equilibrium constant, Kę. The equilibrium constant is written mathematically (for the above equation) as: [C[[D]* K. = [A]°[B]" where, a, b, c, and d are the stoichiometric coefficients from the balanced chemical equation and the brackets, [ ], indicate molar concentration. 1. For the following reaction: 2A + В + 3с calculate the equilibrium constant, K, if at equilibrium the concentration of A is 0.15M, the concentration of B is 0.20M, and the concentration of C is 0.10M.arrow_forwardConsider the following reaction.HSO4 – (aq) + H2O (l) H3O+ (aq) + SO4 2–(aq) Ka = 0.012 If the initial concentrations are [HSO4–] = 0.50 M, [H3O+] = 0.020 M, and [SO4 2–] = 0.060 M, what are the equilibrium concentrations of the products and reactants?arrow_forwardPhosphorus pentachloride decomposes at high temperatures. PC15 (g) ⇒ PC13 (g) + Cl₂ (g) An equilibrium mixture at some temperature consists of 5.72 g of PC15, 4.86 g of PCl3, and 3.59 g of Cl2 in a 1.00-L flask.arrow_forward
- The reaction 2CO(g) + O2(g) = 2 CO2(g) is known to be exothermic. According to Le Chatelier's principle, how will this reaction's equilibrium be affected if the reaction temperature is increased? (A) The equilibrium constant will decrease and the reaction will shift to the left. (B) The equilibrium constant will be unchanged, but the reaction will shift to the left. (C) The equilibrium constant will increase and the reaction will shift to the right. (D) The equilibrium constant will be unchanged, but the reaction will shift to the right. (E) The equilibrium concentrations will not be affected.arrow_forward2:25 1 Question 17 of 25 Submit Consider the equilibrium system described by the chemical reaction below. A 1.00 L reaction vessel was filled 0.0560 mol O, and 0.200 mol N20 and allowed to react at 298 K. At equilibrium, there were 0.0200 mol of NO2 present. Determine the concentrations of all species and then calculate the value of Kc for this reaction. 2 N20(g) + 3 O2(g) =4 NO2(g) 1 2 Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 2 N20(g) + 3 O2(g) = 4 NO2(g) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.0560 0.200 -1.00 -0.0560 0.0200 -0.0200 0.0100 -0.0100 -0.0050 0.0050 0.0150 -0.0150 0.210 0.190 0.0410 0.0710 0.0360 0.180arrow_forwardExactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g). If at equilibrium the N2O4 is 28.0% dissociated, what is the value of the equilibrium constant, Kc, for the reaction under these conditions? (need to show your calculation.)arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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