Chem 1B Final Flashcards by Celaye Pena

Consider the following reaction at equilibrium. What will happen when adding more O2

2 C8H18(g) + 25 O2(g) <—> 18 H2O(l) + 16 CO2(g)

A. the reaction will shift to the left
B. the reaction will shift to the right
C. no change will be observed
D. the equilibrium constant will decrease

B. The reaction will shift to the right

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Express the equilibrium constant for the following reaction: CsIO3(s) <—> CsIO(s) + O2(g)

A. Kc = [O2]
B. Kc = [O2]^-1
C. Kc = [CsIO3]^2/[CsIO]^2[O2]^2
D. Kc = [CsIO][O2]/[CsIO3]

A. Kc = [O2]

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Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [P4O10]eq = 3.000 moles, [P4]eq = 4.000 moles, [O2]eq = 5.000 M

P4O10(s) <—> P4(s) + 5 O2(g)

A. 4167
B. 3125
C. 25.00
D. 5.000

B. 3125

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The following reaction shows the combustion of pentane (C3H8)

C3H8(g) + 5 O2(g) <—> 3 CO2(g) + 4 H2O(l)

What is Δn for the following equation in relating Kc to Kp

A. 3
B. 1
C. -1
D. -3

D. -3

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Consider the following reaction and its equilibrium constant: SO2(g) + NO2(g) <—> SO3(g) + NO(g)
Kc = 0.33
A reaction mixture contains 0.49 M SO2, 0.14 M NO2, 0.12 M SO3, and 0.14 M NO. Which of the following statements is TRUE concerning this system.

A. The system is at equilibrium
B. The reaction will shift in the direction of reactants
C. The reaction will shift in the direction of products
D. The reaction quotient will decrease

C. The reaction will shift in the direction of products

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At 400 K, find the missing Kc

2 SO2(g) + O2(g) <—> 2 SO3(g) Kc = 1.7x10^6
SO3(g) <—> 1/2 O2(g) + SO2(g) Kc = ?

A. 8.5 x10^5
B. 1.3x10^3
C. 7.7x10^-4
D. 5.9x10^-7

C. 7.7x10^-4

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For the isomerization reaction: butane <—> isobutane Kp = 25 at 500 C
If the initial pressures of butane and isobutane are 2.5 atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?

A. P(butane) = 10 atm and P(isobutane) = 1.2atm
B. P(butane) = 2.4 atm and P(isobutane) = 0.096 atm
C. P(butane) = 0.10 atm and P(isobutane) = 2.5 atm
D. P(butane) = 0.096 atm and P(isobutane) = 2.4 atm

D. P(butane) = 0.096 atm and P(isobutane) = 2.4 atm

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The following endothermic reaction is at equilibrium in a sealed container.
PCl3(g) + Cl2(g) <—> PCl5(g) ΔH = 105 kJ
Which of the following changes would result in an increase in the number of moles of PCl5(g) present at equilibrium?

I. increasing the temperature
II. increasing the volume

A. I only
B. II only
C. Both I and II
D. Neither I nor II

A. I only

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Consider the following reaction [N2O4]eq = 0.031 M, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of NO2(g)
N2O4(g) <—> 2 NO2(g) Kc = 0.21

A. 6.5x10^-3 M
B. 8.1x10^-2 M
C. 1.5x10^-1
D. 1.5 M

B. 8.1x10^-2 M

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Determine the value of Kc for the following reaction if the equilibrum concentrations are as follows:
[HCl]eq = 0.13 M, [HI]eq = 5.6x10^-16 M, [Cl2]eq = 0.0019 M

2 HI(g) + Cl2(g) <—> 2 HCl(g) + I2(s)

A. 3.5x10^-32
B. 8.2x10^-18
C. 1.2x10^17
D. 2.8x10^31

D. 2.8x10^31

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Consider the following reaction: COCl2(g) <—> CO(g) + Cl2(g) Kc = 8.33x10^-4
A reaction mixture initially contains 1.6 M COCl2. Determine the equilibrium concentration of CO. Calculate this based on the assumption that the answer is negligible compared to 1.6

A. 2.1x10^-2 M
B. 3.7x10^-2 M
C. 1.5x10^-3 M
D. 4.2x10^-4 M

B. 3.7x10^-2 M

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Which substance is a lewis base?
A. NH3
B. NH4Cl
C. BF3
D. HCl

A. NH3

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Which of the following is a weak base?
A. H2S
B. CH3CO2H
C. NaOH
D. NH(CH3)2

D. NH(CH3)2

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Identify the products that are in equilibrium with NH3 and H2O
A. NH2^- and H3O^+
B. NH3, H^+, and OH^-
C. NH4^+ and OH^-
D. NH2^-, H^+, and H2O

C. NH4^+ and OH^-

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Determine the pH of a 0.00444 M HClO4 solution
A. 1.353
B. 2.353
C. 5.824
D. 11.647

B. 2.353

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Which of the following acid has the greatest percent ionization? The acid is followed by its Ka value.
A. HC6H5O, 1.3x10^-10
B. HOCl, 2.9x10^-8
C. HCHO2, 1.8x10^-4
D. HNO2, 4.6x10^-4

D. HNO2, 4.6x10^-4

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Determine the pH of a 0.461 M benzoic acid (Ka = 6.5x10^-5) solution
A. 9.48
B. 5.48
C. 4.52
D. 2.26

D. 2.26

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Which of the following is TRUE
A. An acidic solution has [H3O^+] > [OH^-]
B. A basic solution does not contain H3O^+
C. A neutral solution contains [H2O] = [H3O^+]
D. An neutral solution does not contain any H3O^+ or OH^-

A. An acidic solution has [H3O^+] > [OH^-]

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What is the conjugate acid of HSO3^-?
A. SO3^-2
B. HSO4^-
C. H2SO3
D. H3O^+

C. H2SO3

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What is the pH of a 0.300 M NH3 solution that has Kb = 1.8 x 10^-5
A. 11.37
B. 10.89
C. 2.63
D. 2.11

A. 11.37

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Which of the following acid is the weakest?
Bases. Kb
NH2CH3. 4.4x10^-4
NH3. 1.8x10^-5
H2NOH. 1.1x10^-8
C5H5N. 1.7x10^-9

A. C5H5NH^+
B. N3NOH^+
C. NH4^+
D. NH3CH3^+

D. NH3Ch3^+

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Which of the following will form an acidic solution in water?
A. KF
B. CaBr2
C. AlCl3
D. NaNO3

C. AlCl3

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Which acid is the strongest?
A. HI
B. HBr
C. HCl
D. HF

A. HI

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Which of the following is a WEAK acid?
A. H2SO4
B. HClO3
C. HCl
D. HI

B. HClO3

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What is the pH of a 0.20 M solution of sodium benzoate, Na(C6H5COO)? The Ka = of benzoic acid, C6H5COOH, is 6.5x10^-5 A. 11.56 B. 9.09 C. 8.74 D. 5.26

C. 8.74

Indicate which of the following mixture will make a buffer solution A. a solution that is 0.10 M CH3COOH and 0.10 M CH3COONa B. A solution that is 0.10 M HF and 0.10 M L CH3COOH C. a solution that is 0.10 M HCl and 0.10 M NH4Cl D. a solution that is 0.10 M NaOH and 0.10 M KOH

A. a solution that is 0.10 M NH3COOH and 0.10 M CH3COONa

What is the pH of a solution that is 0.20 M in HF in and 0.40 M NaF [Ka (HF) = 7.2x10^-4] A. 1.92 B. 2.84 C. 3.14 D. 3.44

D. 3.44

A buffer contains 0.30 mol CH3COOH (Ka = 1.8x10^-5) and 0.50 mole CH3COONa. What's the pH after the addition of 0.05 mol KOH A. 3.96 B. 4.51 C. 5.08 D. 5.42

C. 5.08

A chemist needs a buffer solution at pH 4.30 and has to choose from the following list of acids and their soluble salts, which of them would make the most effective buffer at this pH? A. hypochlorous acid Ka = 3.51x10^-8 B. benzoic acid Ka = 6.40x10^-5 C. chloroacetic acid Ka = 1.35x10^-3 D. nitrous acid Ka = 4.46x10^-2

B. benzoic acid Ka = 6.40x10^-5

Which of the following solutions has the biggest buffer capacity? A. 1.5 M NH3 and 1.5 M NH4^+ B. 0.5 M NH3 and 0.5 M NH4^+ C. 0.1 M NH3 and 0.3 M NH4^+ D. 0.08 M NH3 and 0.5 M NH4^+

A. 1.5 M NH3 and 1.5 M NH4^+

When titrating a monoprotic strong acid with a strong base at 25 C, the A. pH will be 7 at the equivalence point B. pH will be greater than 7 at the equivalence point C. pH will be less than 7 at the equivalence point D. titration will require more moles of the base than acid to reach the equivalence point

A. pH will be 7 at the equivalence point

Determine the molar solubility of AgBr in a solution containing 0.120 M NaBr Ksp (AgBr) = 7.7x10^-13 A. 9.2x10^-14 M B. 6.4x10^-12 M C. 8.8x10^-7 M D. 5.8x10^-5 M

B. 6.4x10^-12 M

A 50.0 mL sample 0.10 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 25.0 mL of KOH. The Ka of HF is 3.5x10^-4 A. 3.15 B. 3.46 C. 4.15 D. 4.33

B. 3.46

What is the [CH3COO^-]/[CH3COOH] ratio necessary to make a buffer solution with a pH of 5.05? (Ka of CH3COOH is 1.8x10^-5) A. 0.50 B. 0.94 C. 1.1 D. 2.0

D. 2.0

What is the molar solubility of magnesium carbonate (MgCO3) in water? The solubility-product constant for MgCO3 is 3.5x10^-8 at 25 C A. 1.8x10^-8 B. 7.0x10^-8 C. 1.9x10^-4 D. 2.6x10^-4

C. 1.9x10^-4

Give the expression for the solubility product constant for BaF2 A. [Ba^2+][F^-]/[BaF2] B. [Ba^2+]^2[F^-] C. [Ba^2+][F^-] D. [Ba^2+][F^-]^2

D. [Ba^2+][F^-]^2

Which of the following will increase the solubility of AgCl(s) A. Addition of AgCl(s) B. Adding NgNO3 C. Adding HNO3 D. Addition of NH3(aq)

Addition of NH3(aq)

A solution containing AgNO3 is mixed with a solution that is 0.10 M in AgNO3 and 0.075 M NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77x10^-10 A. Nothing will happen since the molar solubility of AgCl is higher than the solution concentrations B. Silver chloride will precipitate out of the solution C. Nothing will happen since NaCl and AgNO3 are both soluble compounds D. There is not enough information to say anything about this solution

B. Silver chloride will precipitate out of the solution

Place the following in order of decreasing standard molar entropy N2O4(g). NO(g). NO2(g) A. N2O4 > NO2 > NO B. NO > NO2 > N2O4 C. N2O4 > NO > NO2 D. NO > N2O4 > NO2

A. N2O4 > NO2 > NO

Which reaction has the most positive entropy (ΔS) change under standard conditions? A. H2O(g) + CO(g) ---> H2(g) + CO2(g) B. CaCO3(s) ---> CaO(s) + CO2(g) C. NH3(g) ---> NH3(aq) D. C8H18(l) ---> C8H18(s)

B. CaCO3(s) ---> CaO(s) + CO2(g)

For the reaction: 60 C(s) ---> C60(s) solve for the change in entropy in J/K Given S(C(s)) = 5.7 J/mol-K and S(C60(s)) = 426.0 J/K-mol A. -420.3 B. -84.0 C. 84.0 D. 420.3

C. 84.0

For the following example: Identify the following. H2O(g) ---> H2O(l) A. ΔH = -, ΔS = - B. ΔH = -, ΔS = + C. ΔH = +, ΔS = + D. ΔH = +, ΔS = -

A. ΔH = -, ΔS = -

What are the signs of ΔH and ΔS for a reaction that is spontaneous at all temperatures? A. ΔH is positive, ΔS is positive B. ΔH is positive, ΔS is negative C. ΔH is negative, ΔS is negative D. ΔH is negative, ΔS is positive

D. ΔH is negative, ΔS is positive

Consider the following reaction at constant pressure at 398 K 4 NH3(g) + 3 O2(g) ---> 2 N2(g) + 6 H2O(g) ΔH = -1267 kJ A. ΔSsurr = +50.5 kJ/K, reaction is not spontaneous B. ΔSsurr = +12.67 kJ/K, reaction is not spontaneous C. ΔSsurr = +3.18 kJ/K, reaction is spontaneous D. ΔSsurr = -12.67 kJ/K, reaction is spontaneous

C. ΔSsurr = +3.18 kJ/K, reaction is spontaneous

For a given compound, list the increasing order of entropy for a liquid, solid, and gas A. solid < liquid < gas B. solid < gas < liquid C. liquid < solid < gas D. gas < solid < liquid

A. solid < liquid < gas

Determine ΔGrxn using the following information H2(g) + CO(g) ---> CH2O(g) ΔH = +1.9 kJ; ΔS = -109.6 J/K, T = 298 K A. -41.5 kJ B. -30.8 kJ C. +17.3 kJ D. +34.6 kJ

D. +34.6 kJ

Find the missing ΔG A(g) + B(g) ---> 3 C(g). ΔG = -23kJ 9 C(g) ---> 3 A(g) + 3 B(g). ΔG = ____ A. -69 kJ B. -23 kJ C. -7.67 kJ D. 69 kJ

D. 69 kJ

Which of the following is true for a spontaneous process? I). ΔSsys + ΔSsurr > 0. II). ΔG > 0 A. only I B. only II C. both I and II D. neither I or II

C. both I and II

Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction Fe2O3(s) + 3 CO(g) --->2 Fe(s) + 3 CO2(g) ΔG = -28.0 kJ P(CO) = 1.4 atm, P(CO2) = 2.1 atm A. -30.7 kJ B. -25.0 kJ C. +17.5 kJ D. +31.0 kJ

B. -25.0 kJ

Which of the following reactions will have the largest equilibrium constant (K) at 298 K A. 2 Hg(g) + O2(g) --> 2 HgO(s). ΔG = -180.8 kJ B. Fe2O3(s) + 3 CO(g) --> 2 Fe(s) + 3 CO2(g). ΔG = -28.0 kJ C. CaCO3(s) --> CaO(s) + CO(g). ΔG = +131.1 kJ D. 3 O2(g) --> 2 O3(g). ΔG = +326 kJ

A. 2 Hg(g) + O2(g) --> 2 HgO(s). ΔG = -180.8 kJ

What is the oxidation state of Cl in KClO3? A. -1 B. +1 C. +3 D.+5

D. +5

____ is the reducing agent in the reaction blow Cr2O7^2- + 6 S2O3^2- + 14 H^+ ---> 2Cr^3+ + 3 S4O6^2- + 7H2O A. Cr^3+ B. S4O6^-2 C. S2O3^-2 D. Cr2O7^-2

C. S2O3^2-

what is the coefficient of H^+ when the following equation is balanced? MnO4^- + Br^- ---> Mn^2+ + Br2. (acidic solution) A. 2 B. 16 C. 8 D. 4

B. 16

In a voltaic cell, the half-reaction Ag^+(aq) + e^- ---> Ag(s) is A. an oxidation half-reaction and occurs at the cathode B. a reduction half-reaction and occurs at the cathode C. a reduction half-reaction and occurs at the anode D. an oxidation half-reaction and occurs at the anode

B. a reduction half-reaction and occurs at the cathode

Consider the following table of standard half-cell potentials A2 + 2e^- ---> 2 A. E = +1.09 V B^2+ + 2 e^- ---> B. E = +0.15 V C^3+ + 3 e^- ---> C. E = + 1.66 V D^2+ + 2 e^- ---> D. E = -2.37 V Which substance is the strongest oxidizing agent A. C^3+ B. A2 C. B^4+ D. D^2+

A. C^3+

What is the oxidation half-reaction for the following overall galvanic cell reaction? Pb^2+(aq) + Cu(s) ---> Pb(s) + Cu^2+(aq) A. Cu(s) ---> Cu^2+(aq) + 2e^- B. Cu^2+(aq) + 2e^- ---> Cu(s) C. Pb(s) ---> Pb^2+(aq) + 2e^- D. Pb^2+(aq) + e^- ---> Pb(s)

A. Cu(s) ---> Cu^2+(aq) + 2e^-

For the cell Mg(s) + Cu^2+(aq) ---> Mg^2+ + Cu(s) Which change will increase the voltage of the cell? A. increasing the [Mg^2+] B. increasing the size of the Mg electrode C. increasing the [Cu^2+] D. decreasing the size of the Cu electrode

C. increasing the [Cu^2+]

Use the standard half-cell potentials listed below to calculate the standard cell potential (E°) for the following reaction occurring in an electrochemical cell at 25°C. 2Al(s) + 3Cu2+(aq) → 3Cu(s) + 2Al3+(aq) Al3+(aq) + 3 e⁻ → Al(s) E° = – 1.66 V Cu2+(aq) + 2 e⁻ → Cu(s) E° = + 0.34 V A. +2.00 V B. -2.00 V C. -1.32 V D. +1.32 V

A. +2.00 V

Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq) I2(s) + 2 e⁻ → 2 I⁻(aq) E° = + 0.54 V Fe3+(aq) + 3 e⁻ → Fe(s) E° = – 0.04 V A. –3.4 × 102 kJ B. +4.9 × 101 kJ C. –9.7 × 101 kJ D. +2.3 × 102 kJ

A. –3.4 × 102 kJ

Determine the cell notation for the redox reaction given below. Fe(s) + 2 H⁺(aq) → Fe2+(aq) + H2(g) A. H+(aq) | H2(g) | Pt || Fe (s) | Fe2+(aq) B. H2(g) | H+(aq) | Pt || Fe2+(aq) | Fe (s) C. Fe2+(aq) | Fe(s) || H2(g) | H+(aq) | Pt D. Fe(s) | Fe 2+(aq) || H+(aq) | H2(g) | Pt

D. Fe(s) | Fe 2+(aq) || H+(aq) | H2(g) | Pt

How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution containing Cr3+ ions for 40.0 minutes? A. 3.45 g B. 5.00 g C. 10.3 g D. 0.0575 g

A. 3.45 g

A galvanic cell consists of one half-cell that contains Au(s) and Au 3 +(aq), and one half-cell that contains Cu(s) and Cu2+(aq). What species are produced at the electrodes under standard conditions? Au3+(aq) +3 e⁻ → Au(s) E° = + 1.50 V Cu2+(aq) + 2 e⁻ → Cu(s) E° = + 0.34 V A. Au3+ (aq) is formed at the cathode and, Cu(s) is formed at the anode. B. Au(s) is formed at the cathode, and Cu2+(aq) is formed at the anode. C. Cu(s) is formed at the cathode, and Au 3 +(aq) is formed at the anode. D. Cu2+(aq) is formed at the cathode, and Au(s) is formed at the anode.

B. Au(s) is formed at the cathode, and Cu2+(aq) is formed at the anode.

Which of the following metals will dissolve in HCl? Given activity series: Li > K> Ba> Ca > Mg > Al > Mn > Zn > Cr > Fe > Co > Ni > Sn > H2 > Cu> Ag> Hg > Au A. Hg B. Zn C. Cu D. Ag

B. Zn

How many electrons are transferred after the following reaction is balanced? Al(s) + Cu2+(aq) → Cu(s) + Al3+(aq) A. 6 B. 2 C. 3 D. 1

A. 6

Choose the electron configuration for Cr2+. A. [Ar]3d4 B. [Ar]4s23d4 C. [Ar]4s23d6 D. [Ar]

A. [Ar]3d4

How many unpaired electrons would you expect for the complex ion: [Fe(NO2)6]4⁻ A. 0 B. 2 C. 4 D. 6

A. 0

How many moles of aqueous ions will be produced from the dissolution of 1.0 mole of [Cu(NH3)4]Cl2 in water? A. 1 B. 3 C. 7 D. 5

B. 3

Name the following: [Fe(H2O)4Cl2]Br A. tetraaquadichloro iron(II) bromide B. dichlorotetrahydroiron(II) bromide C. tetraaquadichloro iron(III) bromide D. iron(II) dichlorotetraquabromide

C. tetraaquadichloro iron(III) bromide

Which of the following pairs of coordination compounds are examples of coordination isomers? A. [Cu(NH3)3NO2]Cl2 and [Cu(NH3)3ONO]Cl2 B. [Cu(NH3)2(H2O)2]F2 and [Cu(NH3)2(H2O)2]I2 C. [Cu(NH3)2(H2O)2]Br2 and [Cu(NH3)2(H2O)2]Br2 D. [Cr(CO)5I]Cl and [Cr(CO)5Cl]I

D. [Cr(CO)5I]Cl and [Cr(CO)5Cl]I

Which of the following compounds or complex ions can exhibit cis-trans isomerism? A. [Cr(CO)3(NO2)3 B. [Fe(CO)2(NH3)4]Cl2 C. [MnClBr3]^2- D. [Fe(H2O)6]^3+

B. [Fe(CO)2(NH3)4]Cl2

Which of the following compounds can exhibit fac-mer isomerism? A. [Cr(H2O)4Cl2]^+ B. [Fe(H2O)3(CO)3]^3+ C. [Co(CO)5NO2]^2+ D. [Cu(NH3)2(H2O)4]^2+

B. [Fe(H2O)3(CO)3]^3+

Which ion would you expect to have the smallest crystal field splitting energy Δ? A. [Ni(NO2)6]^3⁻ B. [Ni(CN)6]^3⁻ C. [ Ni(H2O)6]^3+ D. [NiCl6]^3⁻

D. [NiCl6]^3⁻

Identify the geometry of [Co(NH3)6]^3+. A. tetrahedral B. square pyramidal C. trigonal pyramidal D. octahedral

D. octahedral

Which ligand is a bidentate ligand? A. EDTA B. SCN⁻ C. oxalate (C2O4^2-) D. CN⁻

C. oxalate (C2O4^2-)

Which of the following complex ions absorbs light of the shortest wavelength? A. [CoI6]^3⁻ B. [Co(en)3]^3+ C. [Co(OH)6]^3- D. [Co(CN)6]^3⁻

D. [Co(CN)6]^3⁻

An atom of 82 Br undergoes an alpha decay

82 4 78 Br. ---> 𝛼 + As 35 2 33

An atom of Hydrogen-3 undergoes a beta decay

3. 0 3 H ---> 𝛽. +. He 1. -1 2

An atom of 191^Pt undergoes an electron capture

191 0 191 Pt. +. e. --->. Ir 78 -1 77

An atom of Osmium-184 undergoes a positron emission

184 0 184 Os --->. e. + Re 76 1 75

An atom of Californium-255 undergoes three alpha decays and one gamma decay

255. 4. 0. 243 Cf. --->. 3 He. +. 1 𝛾. +. U 98 2 0. 92

A sample of carbon-14 has a half-life of 5730 years. If the mass of the carbon-14 is 455 g today, what will be the mass of the carbon-14 in the sample in 17190 years?

Ln(Nt /N0 ) = -kt t1/2 = 0.693/k so ln( N t /455 g) = - 0.693/5730 yr * 17190 yr Nt = 56.9 g Method 2: 17190/5730 = 3, so three half lives Nt = (½) 3 N0 = (1/2) 3 * 455 g = 56.9 g

Explain fusion and fission

Fusion is when small nuclei smash together to make a larger nucleus Fission is when the large nucleus splits into two smaller nuclei

Chem 1B Final Flashcards

(82 cards)