ISIn the reaction BF-P BK, BF, is acting as what type of acid? a) Arrhenius only

Question

ISIn the reaction BF-P BK, BF, is acting as what type of acid? a) Arrhenius only d) Arrhenius, Bronsted-Lowry, and Lewis b) Lewis o c)Arrhenius and Bronsted-Lowry e) Bronsted-Lowry only 6. Consider the reaction shown here. In an experiment, CO) and H:0(g) are mixed together such a way that their initial concentrations are 0.35 mol/L and 0.40 mol/L respectively (there is no CO, or H: initially present). At cquilibrium it is found that the c moVL. What is the value of the equilibrium constant for this reaction? concentration of CO(g) is 0.19 a) 0.1056 b) 0.56 c)0.34 d) 0.90 e) 0.76 17. Calculate the phi of 0.050 M hypochlorous acid, Ka 3.0 x 10 a)3.87 X10s b) 5.21 c) 7.52 d) 8.94 c) 4.41 a" 18. For the vapor-phase reaction 2AB A2 + B2, Kc = 16 at 523 K. If 0.034 mol AB is introduced into a 1.00 L vessel at 523 K, then at equilibrium [B:] is a) 0.008 M b) 0.003 M c) 0.0052 M d) 024 M e) 0.015 M 19. In the reaction 2NO2 2NO + O2 at 300°C, [NO! drops from 0.100 to 0.030 M in 100 s. What is the average rate of disappearance of NO, for this period in Mis? a) 0.00035 b) 0.000035 c) 0.0018 d) 0.00070 e) 0.0035 2A + 3D products is first-order in A and second-order in D, then the rate law will have the form, rate- 20. If the reaction A B 21. Use the information below to determine the order of the reaction in reactant B Irial ALM [BIM Rate 0.273 0.763 2.83 2 0.273 1526 2.83 3 0819 0.763 25.47 a) 3 c) 2 d) 0 b) I d)4

Explanation / Answer

Arrhenius Acid/Base

Arrhenius acid/base is the first theory on acid/base definitions, it is mostly true for general applications.

Arrhenius acid is any type of substance that will dissociate in water to form hydrogen ions [H+]. That is, an acid increases the concentration of H+ ions in an aqueous solution.

Arrhenius base is any type of substance that will form hydroxide [OH] ions. It typically must increase pH since OH- increases in concentration.

Examples of Arrhenius acid

HCl, H2SO4, H3PO4 à they will donate 1, 2, and 3 protons to solution i.e. H+

Examples of Arrhenius base

NaOH, Ca(OH)2, and; avoid NH3, since it is basic, yet will not donate OH from its NH3 equation.

Bronsted Lowery Acid/Bases

First, let us define Bronsted Lowry acid/base:

Bronsted Lowry acid: any species that will donate H+ (protons) in solution, and makes pH lower (i.e HCl)

Bronsted Lowry base: any species that will accept H+ (protons) in solution, and makes pH higher (NH3 will accept H+ to form NH4+)

Typically, acid/bases are shown in the left (reactants)

when we write the products:

Bronsted Lowery conjugate base = the base formed when the B.L. acid donates its H+ proton ( i.e. HCl -> Cl-

Bronsted Lowery conjugate acid = the acid formed when the B.L. base accept its H+ proton ( i.e. NH4+ has accept H+ proton)

Note that, typically conjugate bases/acids are shown in the right (product) side

Lewis Acid/Base

Lewis acid and base theory deals mainly with electron transfer, rather than proton transfer (H+).

A Lewis acid will accept an electron pair

A Lewis base will donate an electron pair

Examples of a Lewis base:

Anything that will accept negatively charged species will do, such as halides, complex anions, etc…

Examples of a Lewis acid:

BH3, AlCl3, FeCl3, H+

therefore,

this can't be ahrrenius, no OH- and H+ rpresent

this cant be Bronsted Lowry, since it has no H+ exchange

therefore, this is lewis only

Q16

initially

[CO] = 0.35

[H2O] = 0.40

[CO2] = 0

[H2] = 0

in equilbirium

[CO] = 0.35-x

[H2O] = 0.40-x

[CO2] = 0+x

[H2] = 0 +x

and we know

[CO] = 0.35-x = 0.19

x = 0.35-0.19 = 0.16

[H2O] = 0.40-0.16 = 0.24

[CO2] = 0+0.16 = 0.16

[H2] = 0 +0.16 = 0.16

KP = (CO2)(H2)/((CO*H2O))

Kp = (0.16*0.16)/(0.24*0.19)

Kp = 0.5614

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