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Chemistry
Q:
Identify the set of Lewis acids.
A) BH3, BF3, Cu2+, CO2
B) Cl-, OH-, NH3, H2O
C) H3PO4, H2PO4-, HPO42-, PO43-
D) CH3-, NH2-, OH-, F-
Q:
The compound BF3 can be described as a(n)
A) Arrhenius acid.
B) Brnsted-Lowry acid.
C) Lewis acid.
D) Lewis base.
Q:
Which one of the following is least able to behave as a Lewis base?
A) CH3NH2
B) (CH3)2NH
C) (CH3)3N
D) (CH3)3NH+
Q:
Which one of the following is not considered to be a Lewis base?
A) H2O
B) NH3
C) NH4+
D) Cl-
Q:
For Cu2+ and CO2, which will behave as a Lewis acid toward OH- in water?
A) only Cu2+
B) only CO2
C) Cu2+ and CO2
D) neither Cu2+ nor CO2
Q:
Identify the Lewis acid that acts as a reactant in the following reactionCo(H2O)63+(aq) + 6 NH3(aq) -> Co(NH3)63+(aq) + 6 H2O(l).A) Co(H2O)63+B) Co3+C) NH3D) H2O
Q:
Identify the Lewis acid that acts as a reactant in the following reaction
Fe(H2O)63+(aq) + 6 CN-(aq) → Fe(CN)63-(aq) + 6 H2O(l).
A) Fe3+
B) H2O
C) CN-
D) Fe(H2O)63+
Q:
What is the strongest acid among the following?
A) CH3CO2H
B) ClCH2CO2H
C) Cl2CHCO2H
D) Cl3CCO2H
Q:
What is the strongest acid among the following?
A) HIO
B) HIO2
C) HIO3
D) HIO4
Q:
What is the strongest acid of the following?
A) HOI
B) HOBr
C) HOCl
D) All are equivalent.
Q:
What is the strongest acid among the following?
A) H2SO3
B) H2SO4
C) H2SeO3
D) H2SeO4
Q:
What is the strongest base among the following?
A) ClO-
B) ClO2-
C) ClO3-
D) ClO4-
Q:
Which acid of the following set has the strongest conjugate base?
A) CH4
B) NH3
C) H2O
D) HF
Q:
What is the weakest acid among the following?
A) SiH4
B) PH3
C) H2S
D) HCl
Q:
What is the strongest acid among the following?
A) HF
B) HCl
C) H2O
D) H2S
Q:
What is the strongest acid among the following?
A) H2O
B) H2S
C) H2Se
D) H2Te
Q:
What is the strongest acid among the following?
A) HF
B) HCl
C) HBr
D) HI
Q:
What is the identity of M in the hydrate M(H2O)6n+ that has the 0.10 M solution with the highest pH?
A) Li+
B) Na+
C) Mg2+
D) Al3+
Q:
What is the identity of M in the hydrate M(H2O)6n+ that has the 0.10 M solution with the lowest pH?
A) Li+
B) Na+
C) Mg2+
D) Al3+
Q:
Which one of the following salts, when dissolved in water, produces the solution with the lowest pH?
A) NaCl
B) NH4Cl
C) MgCl2
D) AlCl3
Q:
Nitric oxide reacts with oxygen to form nitrogen dioxide:2 NO(g) + O2(g) 2 NO2(g)What is Kc for the forward reaction if the equilibrium concentration of NO is 0.200 M, O2 is 0.100 M, and NO2 is 0.250 M at 25C?A) 8.00 10-2B) 6.41 10-2C) 12.5D) 15.6
Q:
Write the equilibrium constant expression for the following reaction in the reverse direction:2 CH4 (g) + 3 O2 (g) 2 CO (g) + 4 H2O (g)A) Kc' = B) Kc' = C) Kc' = D) Kc' =
Q:
Write the equilibrium constant expression for the following reaction in the forward direction:2 CH4 (g) + 3 O2 (g) 2 CO (g) + 4 H2O (g)A) Kc = B) Kc = C) Kc = D) Kc =
Q:
If Kc is the equilibrium constant for a forward reaction, 2 A B, what is Kc- for the reaction 4 A 2B?A) KcB) KcC) 2 KcD) (Kc)2
Q:
If Kc is the equilibrium constant for a forward reaction what is Kc' for the reverse reaction?
A) -Kc
B) Kc
C) (Kc)-1
D) none of these
Q:
Which statement about the equilibrium constant is true? The value of Kc
A) changes as product concentration changes.
B) changes as reactant concentration changes.
C) changes as temperature changes.
D) never changes.
Q:
Which of the following statements is false regarding the equilibrium constant, Kc?
A) Kc for a reaction at a particular temperature always has the same value.
B) Kc for the reverse reaction is the negative of Kc for the forward reaction.
C) The numerical value of Kc depends on the form of the balanced equation.
D) When quoting Kc it is customary to omit units.
Q:
The equilibrium equation is also known as the law of
A) coefficients.
B) constant concentration.
C) dynamic equilibrium.
D) mass action.
Q:
Which one of the following statements does not describe the equilibrium state?
A) Equilibrium is dynamic and there is no net conversion to reactants and products.
B) The concentration of the reactants is equal to the concentration of the products.
C) The concentration of the reactants and products reach a constant level.
D) The rate of the forward reaction is equal to the rate of the reverse reaction.
Q:
The reaction below is heated from 20C to 90C, according to Le Chtelier's principle, there will be a net reaction from ________ to ________, and the brown color will become ________.N2O4(g) 2 NO2(g)H= + 57.2 kJcolorless brown
Q:
According to Le Chtelier's principle, if the volume of the vessel containing the equilibrium system shown below is decreased, there will be an increase in the concentration of ________ and a decrease in the concentration of ________.H2(g) 2 H(g)
Q:
If additional SCN- is added to the equilibrium system shown below, Le Chtelier's principle predicts a net reaction from ________ to ________, causing the red color to become ________.Fe3+(aq) + SCN-(aq) FeSCN2+(aq)yellow colorless red
Q:
Kc = 1.2 10-42 at 500 K for the reaction shown below.H2(g) 2 H(g)If [H2] = 1 10-2 M and [H] = 1.2 10-22 M, in order to achieve equilibrium a net reaction must occur from ________ to ________ until Qc = ________.
Q:
Kc = 57.0at 700 K for the reaction shown below.H2(g) + I2(g) 2 HI(g)If [H2(g)] = [I2(g)] = 0.200 M at equilibrium, the molar concentration [HI((g)] = ________ at equilibrium.
Q:
For the reaction shown below the equilibrium constant expression for Kc = ________.HF(aq) + H2O(l) H3O+(aq) + F-(aq)
Q:
For the reaction shown below the value of Kp is ________ than the value of Kc, because n = ________.N2O4(g) 2 NO2(g)
Q:
For the reaction shown below, N2O4 and NO2 have equilibrium concentrations, [N2O4]eq = 2.160 10-4 and [NO2]eq = 1.001 10-3, respectively. The equilibrium constant, Kc, for this reaction equals ________.N2O4(g) 2 NO2(g)
Q:
In a reversible reaction, when the rate of the forward reaction equals the rate of the reverse reaction, the reaction is at ________.
Q:
A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.
Q:
Kc is 1.67 1020 at 25C for the formation of iron(III) oxalate complex ion:Fe3+(aq) + 3 C2O42-(aq) [Fe(C2O4)3]3-(aq).If 0.0400 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium?A) 3.51 10-22 MB) 0.0100 MC) 4.18 1017 MD) 2.85 1021 M
Q:
Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: At 250 0.125 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?
A) [PCl5] = 0.00765 M, [PCl3] = 0.117 M, and [Cl2] = 0.117 M
B) [PCl5] = 0.0625 M, [PCl3] = 0.335 M, and [Cl2] = 0.335 M
C) [PCl5] = 1.80 M, [PCl3] = 1.80 M, and [Cl2] = 1.80 M
D) [PCl5] = 3.96 M, [PCl3] = 3.83 M, and [Cl2] = 3.83 M
Q:
The equilibrium constant, Kp, equals 3.40 for the isomerization reaction:cis-2-butene trans-2-butene.If a flask initially contains 0.250 atm of cis-2-butene and 0.145 atm of trans-2-butene, what is the equilibrium pressure of each gas?A) P(cis-2-butene) = 0.0426 atm and P(trans-2-butene) = 0.145 atmB) P(cis-2-butene) = 0.0471 atm and P(trans-2-butene) = 0.160 atmC) P(cis-2-butene) = 0.0735 atm and P(trans-2-butene) = 0.250 atmD) P(cis-2-butene) = 0.0898 atm and P(trans-2-butene) = 0.305 atm
Q:
At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction:2 ICl(g) I2(g) + Cl2(g).What is the equilibrium concentration of ICl if 0.75 mol of I2 and 0.75 mol of Cl2 are initially mixed in a 2.0-L flask?A) 0.22 MB) 0.28 MC) 0.45 MD) 0.56 M
Q:
Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation:C6H12 CH3C5H9If Kc = 0.143 at 25C for this reaction, find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 M and 0.075 M, respectively.A) [C6H12] = 0.041 M, [CH3C5H9] = 0.041 MB) [C6H12] = 0.159 M, [CH3C5H9] = 0.116 MC) [C6H12] = 0.241 M, [CH3C5H9] = 0.034 MD) [C6H12] = 0.253 M, [CH3C5H9] = 0.022 M
Q:
For the isomerization reaction:butane isobutaneKp equals 25 at 500C. If the initial pressures of butane and isobutane are 20. atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?A) P(butane) = 0.77 atm and P(isobutane) = 19.2 atmB) P(butane) = 0.80 atm and P(isobutane) = 20. atmC) P(butane) = 19.2 atm and P(isobutane) = 0.77 atmD) P(butane) = 20 atm and P(isobutane) = 0.80 atm
Q:
At a certain temperature, Kc equals 1.4 102 for the reaction:2 CO(g) + O2(g) 2 CO2(g).If a 3.00-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium, how many moles of CO are also present in the flask?A) 0.555 molB) 0.185 molC) 0.107 molD) 0.0114 mol
Q:
The equilibrium constant, , is equal to 1.4 at 1200 K for the reaction:C(g) + (g) CO(g) + O(g)If 0.50 moles of C and 0.60 moles of are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached?A) 0.30 MB) 0.21 MC) 0.35 MD) 0.55M
Q:
The equilibrium constant, , is equal to 1.4 at 1200 K for the reaction:C(g) + (g) CO(g) + O(g)If 0.50 moles of C and 0.60 moles of are introduced into a 1.0-L flask, what will be the concentration of C when equilibrium is reached?A) 0.30 MB) 0.21 MC) 0.35 MD) 0.55M
Q:
The equilibrium constant, , is equal to 1.4 at 1200 K for the reaction:C(g) + (g) CO(g) + O(g)If 0.65 moles of C and 0.65 moles of are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached?A) 0.30 MB) 0.35 MC) 0.38 MD) 0.42M
Q:
The equilibrium constant, , is equal to 1.4 at 1200 K for the reaction:C(g) + (g) CO(g) + O(g)If 0.75 moles of C and 0.75 moles of are introduced into a 1.0-L flask, what will be the concentration of C when equilibrium is reached?A) 0.34 MB) 0.41 MC) 0.44 MD) 0.51M
Q:
The equilibrium constant, , is equal to 2.00 at 1000 C for the reaction:2CO(g) C(g) + C(g)If 2.0 moles of CO is introduced into in a 1.0-L flask, what will be the concentration of C when equilibrium is reached?A) 0.74 MB) 0.52 MC) 1.01 MD) 0.78 M
Q:
The equilibrium constant, , is equal to 2.00 at 1000 C for the reaction:2CO(g) C(g) + C(g)If 0.079moles of C and 0.079 moles of C are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached?A) 0.041 MB) 0.058 MC) 0.021 MD) 0.025 M
Q:
An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0100 M O2. At this temperature, Kc equals 1.4 102 for the reaction:2 CO(g) + O2(g) 2 CO2(g).What is the equilibrium concentration of CO?A) 7.1 10-7 MB) 8.4 10-4 MC) 1.4 10-2 MD) 1.2 10-1 M
Q:
At a certain temperature, nitrogen and hydrogen react to form ammonia:N2(g) + 3 H2(g) 2 NH3(g).When initial amounts of N2, H2, and NH3 are mixed, the concentration of NH3 increases. Which statement below is true?A) Kc < QB) Kc > QC) Kc = QD) More information is needed to make a statement about Kc.
Q:
Cyclohexane (C6H12) undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane (MCP) according to the equation:C6H12 MCPIf Kc = 0.143 at 25C for this reaction, predict the direction in which the system will shift if the initial concentrations of C6H12 and MCP are 0.0400 M and 0.0200 M, respectively. The systemA) will shift left.B) will shift right.C) is already at equilibrium.D) is not at equilibrium and will remain in an unequilibrated state.
Q:
The equilibrium constant, Kp, equals 3.40 at 25C for the isomerization reaction:cis-2-butene trans-2-butene.If a flask initially contains 5.00 atm of each gas, in what direction will the system shift to reach equilibrium?A) It will shift left.B) It will shift right.C) The system is already at equilibrium.D) The system is not at equilibrium and will remain in an unequilibrated state.
Q:
The equilibrium constant is equal to 5.00 at 1300 K for the reaction:2 SO2(g) + O2(g) 2 SO3(g).If initial concentrations are [SO2] = 6.00 M, [O2] = 0.45 M, and [SO3] = 9.00 M, the system isA) at equilibrium.B) not at equilibrium and will remain in an unequilibrated state.C) not at equilibrium and will shift to the left to achieve an equilibrium state.D) not at equilibrium and will shift to the right to achieve an equilibrium state.
Q:
For the reaction: N2(g) + 2 O2(g) 2 NO2(g), Kc = 8.3 10-10 at 25C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?A) 3.3 10-11 MB) 1.7 10-10 MC) 6.0 109 MD) 3.0 1010 M
Q:
Which picture (2)-(4) represents the equilibrium mixture when more solid CaO is added?A) picture (2)B) picture (3)C) picture (4)D) all of the above
Q:
Which picture (2)-(4) represents the equilibrium mixture when more solid CaCO3 is added?
A) picture (2)
B) picture (3)
C) picture (4)
D) all of the above
Q:
Which picture (2)-(4) represents the equilibrium mixture when a catalyst is added?
A) picture (2)
B) picture (3)
C) picture (4)
D) all of the above
Q:
Which picture (2)-(4) represents the equilibrium mixture at a higher temperature?
A) picture (2)
B) picture (3)
C) picture (4)
D) none of the above
Q:
Picture (1) represents an equilibrium mixture of solid CaCO3, solid CaO, and gaseous CO2, obtained as a result of the endothermic decomposition of CaCO3.Which picture (2)-(4) represents the equilibrium mixture after addition of four more CO2 molecules?A) picture (2)B) picture (3)C) picture (4)D) none of the above
Q:
Picture (1) represents the equilibrium mixture for the gas-phase reaction A + B 2 AB at 298 K. If the volume of the equilibrium mixture is decreased, which picture (2)-(4) represents the equilibrium at the reduced volume?A) picture (2)B) picture (3)C) picture (4)D) none of the above
Q:
If this reaction is endothermic, which picture (2)-(4) represents the equilibrium mixture at 400 K?
A) picture (2)
B) picture (3)
C) picture (4)
D) none of the above
Q:
Picture (1) represents the equilibrium mixture for the reaction A + B ⇌ 2 AB at 298 K.If this reaction is exothermic, which picture (2)-(4) represents the equilibrium mixture at 400 K?A) picture (2)B) picture (3)C) picture (4)D) none of the above
Q:
Consider the reaction A + B ⇌ 2 AB. The vessel on the right contains an equilibrium mixture of A atoms (shaded spheres), B atoms (unshaded spheres), and AB molecules.If the barrier between the two vessels is removed and the contents of the two vessels are allowed to mix, what will be observed?A) The reaction will go in the forward direction decreasing the number of A atoms and B atoms and increasing the number of AB molecules.B) The reaction will go in the forward direction increasing the number of A atoms and B atoms and decreasing the number of AB molecules.C) The reaction will go in the reverse direction decreasing the number of A atoms and B atoms and increasing the number of AB molecules.D) The reaction will go in the reverse direction increasing the number of A atoms and B atoms and decreasing the number of AB molecules.
Q:
If the volume of the equilibrium mixture is decreased, what will happen to the number of AB molecules and the number of B atoms?A) The number of AB molecules and the number of B atoms will both decrease.B) The number of AB molecules will increase; the number of B atoms will decrease.C) The number of AB molecules will decrease; the number of B atoms will increase.D) The number of AB molecules and the number of B atoms will both increase.
Q:
The following pictures represent the initial state and the equilibrium state for the gaseous state reaction of A2 molecules (shaded spheres) with B atoms (unshaded spheres) to give AB molecules.What is the best balanced chemical equation for the reaction?A) A2 + B A2BB) 1A2 + 2 B A2B2C) A2 + 2 B 2 ABD) 6 A2 + 9 B 3 A2 + 3B + 6 AB
Q:
Which nonequilibrium mixtures will react in the reverse direction to reach equilibrium?A) reaction mixtures (1) and (2)B) reaction mixtures (1) and (4)C) reaction mixtures (2) and (3)D) reaction mixtures (3) and (4)
Q:
The reaction A2 + B2 2AB has an equilibrium constant Kc = 1.8. The following pictures represent reaction mixtures that contain A2 molecules (shaded) and B2 molecules (unshaded), and AB molecules.Which nonequilibrium mixture will react in the forward direction to reach equilibrium?A) reaction mixture (1)B) reaction mixture (2)C) reaction mixture (3)D) reaction mixture (4)
Q:
The following picture represents the equilibrium state for the reaction A2 + B2 2AB. What is the relationship between the rate constant for the forward reaction, kf, and the rate constant for the reverse reaction kr?A) kf < krB) kf = kr = 0C) kf = krD) kf > kr
Q:
The following picture represents the equilibrium state for the reaction A2 + B2 2AB. What is the relationship between the rate constant for the forward reaction, kf, and the rate constant for the reverse reaction kr?A) kf < krB) kf = kr = 0C) kf = krD) kf > kr
Q:
The following picture represents the equilibrium state for the reaction A2 + B2 2AB. What is the relationship between the rate constant for the forward reaction, kf, and the rate constant for the reverse reaction kr?A) kf < krB) kf = kr = 0C) kf = krD) kf > kr
Q:
Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant isA) Kc < 1.B) Kc = 0.C) Kc = 1.D) Kc > 1.
Q:
Shown below is a concentration vs. time plot for the reaction A ⇌ B. For this reaction the value of the equilibrium constant is A) Kc < 1.
B) Kc = 0.
C) Kc = 1.
D) Kc > 1.
Q:
Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant isA) Kc < 1.B) Kc = 0.C) Kc = 1.D) Kc > 1.
Q:
Shown below is a concentration vs. time plot for the reaction A B. For this reaction the value of the equilibrium constant isA) Kc < 1.B) Kc = 0.C) Kc = 1.D) Kc > 1.
Q:
Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant isA) Kc < 1.B) Kc = 0.C) Kc = 1.D) Kc > 1.
Q:
Shown below is a concentration vs. time plot for the reaction A B. For this reaction the value of the equilibrium constant isA) Kc < 1.B) Kc = 0.C) Kc = 1.D) Kc > 1.