Pls help. 5) For the reaction CO(g) + NO2(g) → CO2(g) + NO(g), which result will occur if the container experiences adecrease in volume.a. There will be no effect on the systemb. The reaction will shift to the left.c. The reaction will shift to the right.d. The reaction will heat up.6) In the following reaction, what are the two Bronsted-Lowry bases?a. NH3 and HC1b. NH3 and Clc. HCl and Cl-d. HCl and NH4+NH3(aq) + HCl(aq) ↔ NH4+ (aq) + Cl(aq)

Answered: Image /qna-images/answer/b0b5db25-9ddc-4772-bf90-7e33a9e3928f.jpg

Answered: 5) For the reaction CO(g) + NO2(g) →…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 17CR: . a. Write the conjugate acid for each of the following Brønsted-Lowry bases....

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Similar questions

Most naturally occurring acids are weak acids. Lactic acid is one example. CH3CH(OH)CO2H(s)+H2O(l)H3O+(aq)+CH3CH(OH)CO2(aq) If you place some lactic acid in water, it will ionize to a small extent, and an equilibrium will be established. Suggest some experiments to prow that this is a weak acid and that the establishment of equilibrium is a reversible process.
Calculate the concentration of all solute species in each of the following solutions of acids or bases. Assume that the ionization of water can be neglected, and show that the change in the initial concentrations can be neglected, Ionization constants can be found in Appendix H and Appendix I. (a) 0.0092 M HCIO, a weak acid. (b) 0.0784 M C6H5NH2, a weak base. (c) 0.0810 M HCN, a weak acid. (d) 0.11 M (CH3)3N, a weak base. (e) 0.120 M Fe(H2O)62+ a weak acid, Ka=1.6107
Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.
Consider the following statements. Write out an example reaction and K expression that is associated with each statement. a. The autoionization of water. b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion. c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion.
a. Write the conjugate base for each of the following Brensted- Lowry acids. Oj, H2SOj. HC1O4. NH/. H2CO, Write the conjugate acid for each of the following Bronsted- Lowry bases. ~. hso4- nh2- nh3, co32-
Hydrazine, N2H4, can interact with water in two steps. N2H4(aq) + H2O() N2H5+(aq) + OH(aq) Kb1 = 8.5 107 N2H5+(aq) + H2O() N2H62+(aq) + OH(aq) Kb2 = 8.9 1016 (a) What is the concentration of OH, N2H5+ and N2H62+ in a 0.010M aqueous solution of hydrazine? (b) What is the pH of the 0.010M solution hydrazine?
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
Acetic acid and sodium hydrogen carbonate, NaHCO3, are mixed in water. Write a balanced equation for the acid-base reaction that could, in principle, occur. Using Table 16.2, decide whether the equilibrium lies predominantly to the right or to the left.
The structure of ethylene diamine is illustrated in study question 76. Is this compound a Brnsted acid, a Brnsted base, a Lewis acid or a Lewis base, or some combination of these.
Write chemical equations that show the indicated behavior in aqueous solution for each of the following chemical species. a. HOCl behaves as a BrnstedLowry acid b. NH3 behaves as a BrnstedLowry base c. H2PO4 behaves as a BrnstedLowry acid d. CO32 behaves as a BrnstedLowry base
Boron trifluoride, BF3, and ammonia, NH3, react to produce BF3: NH3. A coordinate covalent bond is formed between the boron atom on BF3 and the nitrogen atom on NH3. Write the equation for this reaction, using Lewis electron-dot formulas. Label the Lewis acid and the Lewis base. Determine how many grams of BF3: NH3 are formed when 10.0 g BF3 and 10.0 g NH3 are placed in a reaction vessel, assuming that the reaction goes to completion.
5. Given the general equation illustrating the reaction of the acid HA in water, HA(aq)+H2O(l)H3O+(aq)+A(aq)explain why water is considered a base in the Brønsted-Lowry model.

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