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Chemistry
Q:
The following pictures represent mixtures of A2B4 molecules and AB2 molecules, which interconvert according to the equation A2B4 2 AB2. If mixture (1) is at equilibrium, which of the other mixtures are also at equilibrium?A) mixture (2)B) mixture (3)C) mixture (4)D) None of the other mixtures are at equilibrium.
Q:
The following pictures represent mixtures of A2B4 molecules and AB2 molecules, which interconvert according to the equation A2B4 2 AB2. If mixture (1) is at equilibrium, which of the other mixtures are also at equilibrium?A) mixture (2)B) mixture (3)C) mixture (4)D) None of the other mixtures are at equilibrium.
Q:
The following pictures represent mixtures of cis-C2H2X2 molecules and trans-C2H2X2 molecules, which interconvert according to the equation cis-C2H2X2 trans-C2H2X2. If mixture (1) is at equilibrium, which of the other mixtures are also at equilibrium?A) mixture (2)B) mixture (3)C) mixture (4)D) None of the other mixtures are at equilibrium.
Q:
The following pictures represent mixtures of cis-C2H2X2 molecules and trans-C2H2X2 molecules, which interconvert according to the equation cis-C2H2X2 trans-C2H2X2. If mixture (1) is at equilibrium, which of the other mixtures are also at equilibrium?A) mixture (2)B) mixture (3)C) mixture (4)D) None of the other mixtures are at equilibrium.
Q:
The reaction A2 + B2 2 AB 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 reaction mixture is at equilibrium?A) reaction mixture (1)B) reaction mixture (2)C) reaction mixture (3)D) reaction mixture (4)
Q:
Which reaction has the smallest equilibrium constant?A) A2 + B2 2 ABB) A2 + C2 2 ACC) A2 + D2 2 ADD) A2 + E2 2 AE
Q:
The following pictures represent the equilibrium state for four different reactions of the type A atoms are unshaded. X atoms are shaded.Which reaction has the largest equilibrium constant?A) A2 + B2 2 ABB) A2 + C2 2 ACC) A2 + D2 2 ADD) A2 + E2 2 AE
Q:
What is the value of the equilibrium constant Kc for the reaction A B?A) Kc = 0.33B) Kc = 3.0C) Kc = 12D) 2Kc = 27
Q:
Consider the interconversion of A molecules (shaded spheres) and B molecules (unshaded spheres) according to the reaction A ⇌ B. Each of the following series of pictures represents a separate experiment in which time increases from left to right.Which of these experiments has resulted in an equilibrium state?A) all of the experiments except experiment (1)B) all of the experiments except experiment (2)C) all of the experiments except experiment (3)D) all of the experiments except experiment (4)
Q:
The reaction below virtually goes to completion because cyanide ion forms very stable complexes with Ni2+ ion:[Ni(H2O)6]2+(aq) + 4 CN-(aq) [Ni(CN)4]2-(aq) + 6 H2O(l)At the same time, incorporation of 14C labelled cyanide ion (14CN-) is very rapid:[Ni(CN)4]2-(aq) + 4 14CN-(aq) = [Ni(14CN)4]2-(aq) + 4 CN-(aq)Which statement below is correct with regard to stability and rate of reaction?A) Equilibrium is static.B) Stable species can react rapidly.C) Stable species do not react rapidly.D) Unstable species react rapidly.
Q:
The hexaammine cobalt(III) ion is very unstable in acidic aqueous solution:[Co(NH3)6]3+(aq) + 6 H3O+(aq) [Co(H2O)6]4+(aq) + 6 NH4+(aq)However, solutions of hexaammine cobalt(III) can be stored in acidic solution for months without noticeable decomposition. Which statement below about the equilibrium constant and the activation energy for the reaction is true?A) Keq < 103 and Ea is very small.B) Keq > 103 and Ea is very small.C) Keq < 103 and Ea is very large.D) Keq > 103 and Ea is very large.
Q:
Nickel metal can be prepared by the reduction of nickel oxide:NiO(s) + CO(g) CO2(g) + Ni(s)At 936 K, Kp = 4.54 103 and at 1125 K, Kp = 1.58 103. Which statement is true?A) The activation energy decreases with increasing temperature.B) The activation energy increases with increasing temperature.C) The reaction is endothermic.D) The reaction is exothermic.
Q:
At 25C, a certain first order reaction has a rate constant equal to 1.00 10-3 s-1 and an equilibrium constant, Kc, equal to 4.18. What is the rate constant for the reverse reaction?
A) 2.39 10-4 s-1
B) 34.18 10-3 s-1
C) 2.39 102 s-1
D) 4.18 103 s-1
Q:
Find the equilibrium constant for the reaction: at 25C when k equals for the reaction at 25C and k equals for the reaction: A) 3.8 10-25
B) 1.7 10-12
C) 1.1 10-12
D) 5.2
Q:
A reaction reaches dynamic equilibrium at a given temperature when
A) the amount of products exceeds the amount of reactants.
B) kfwd equals krev.
C) opposing reactions cease and the system is static.
D) the relative amounts of reactants and products are constant and ratefwd = raterev.
Q:
A catalyst increases the rate of a chemical reaction by providing a lower-energy mechanism for the reaction. When this occurs, which one of the following is not affected?
A) activation energy for the forward reaction
B) activation energy for the reverse reaction
C) equilibrium constant
D) rate of the reverse reaction
Q:
A catalyst increases the overall rate of reaction by lowering the activation energy, Ea, for
A) both the forward reaction and the reverse reaction.
B) neither the forward reaction nor the reverse reaction.
C) only the forward reaction.
D) only the reverse reaction.
Q:
Which of the following statements about a catalyst is true?
A) A catalyst changes the position of the equilibrium in a reaction.
B) A catalyst increases the temperature of a reaction.
C) A catalyst is consumed in a chemical reaction.
D) A catalyst provides a lower energy pathway for a reaction.
Q:
Which of the following changes in reaction conditions will not alter the composition of a homogeneous equilibrium mixture of gases in a reaction having unequal moles of gaseous products and reactants?
A) addition of a catalyst
B) addition of reactants or products
C) decreasing the temperature
D) increasing the pressure or volume
Q:
The decomposition of nitrosyl bromide is exothermic: 2 NOBr(g) 2 NO(g) + Br2(g). Which of the following changes in reaction condition will shift the reaction to the left?A) add more NOBrB) decrease the temperatureC) increase the container volumeD) none of the above
Q:
Calcium carbonate is relatively insoluble and the dissolution reaction is endothermic: CaCO3(s) Ca2+(aq) + CO32-(aq). Which change in reaction condition below will shift the equilibrium to the right?A) add an acid to react with CO32- ionB) add an anion with which Ca2+ is even less soluble than calcium carbonateC) increase the temperatureD) All of the above will shift reaction to the right.
Q:
The dissolution of calcium hydroxide is exothermic.Ca(OH)2(s) Ca2+(aq) + 2 OH-(aq) What happens when the solution of Ca(OH)2 is heated?A) The amount of Ca(OH)2(s) decreases.B) The amount of Ca(OH)2(s) increases.C) The amount of Ca(OH)2(s) remains unchanged.D) The Ca(OH)2(s) completely dissolves.
Q:
The overall reaction for photosynthesis can be represented by the following equation:6 CO2(g) + 6 H2O(l) C6H12O6(s) + 6 O2(g)The enthalpy change for this reaction is 2802 kJ. Which of the following changes in condition will shift the equilibrium to the right?A) increase the pressure of O2B) increase the temperatureC) remove CO2 by reaction with CaO(s)D) remove one-half of C6H12O6(s)
Q:
For the reaction shown below, which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product?C(s) + 2 H2(g) CH4(g) H = - 74.8 kJA) adding more CB) increasing the volumeC) lowering the temperatureD) raising the temperature
Q:
Ammonium bromide is a crystalline solid that decomposes endothermically when heated: NH4Br(s) NH3(g) + HBr(g). When solid NH4Br is added to an evacuated flask at 300C, which change in reaction conditions below will cause the equilibrium to shift to the right?A) add more NH3B) add more NH4BrC) decrease the temperatureD) double the volume of the container
Q:
Which change in the system will drive equilibrium to the left in the reaction below?N2O5(g) NO2(g) + NO3(g)A) decrease the amount of NO3B) increase the amount of N2O5C) increase the pressureD) increase the volume
Q:
For the reaction shown below, which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product?C(s) + 2 H2(g) CH4(g) H = -74.8 kJA) adding HeB) adding more CC) decreasing the volumeD) increasing the volume
Q:
A crude type of disappearing ink is based on the following endothermic equilibrium:[Co(H2O)6]Cl2 (aq) [CoCl2(H2O)4] (aq) + 2 H2O (l)(colorless) (blue)If the reactant solution is used to on a piece of paper and the paper is allowed to partially dry, what can be done to bring out the colored handwriting?A) add waterB) decrease the volumeC) put the paper in a freezerD) put the paper in an oven
Q:
The enthalpy for the following reaction is 136 kJ. If the reaction takes place in a closed container, which one of the following reaction conditions will not decrease the concentration of water vapor?2 NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g)A) add CO2B) cool the containerC) decrease the volume of the containerD) remove some NaHCO3
Q:
Iron oxide ores are reduced to iron metal by exothermic reaction with carbon monoxide: Which of the following changes in condition will cause the equilibrium to shift to the right?
A) add FeO
B) add CO
C) add CO2
D) raise the temperature
Q:
The pink and blue species below form a violet colored mixture at equilibrium:[Co(H2O)6]2+ (aq) + 4 Cl- (aq) [CoCl4]2- (aq) + 6 H2O (l)(pink) (blue)If the concentration of [Co(H2O)6]2+ is increased, what happens to the solution?A) The concentration of [CoCl4]2- increases.B) The concentration of [CoCl4]2- decreases.C) The solution becomes colorless.D) No color change is observed.
Q:
For the reaction shown below, which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product?C(s) + 2 H2(g) CH4(g) H = - 74.8 kJA) adding more CB) decreasing the concentration of H2C) increasing the concentration of H2D) increasing the concentration of CH4
Q:
For a homogeneous equilibrium of gases, which of the following changes in reaction conditions will not alter the equilibrium concentrations?
A) addition of an inert gas to the reaction mixture
B) addition of reactants or products
C) decreasing the pressure or volume
D) increasing the temperature
Q:
Which of the following changes in reaction conditions will alter the composition of an equilibrium mixture of gases for a reaction having unequal moles of gaseous products and gaseous reactants?
A) addition of reactants or products
B) decreasing the pressure or volume
C) increasing the temperature
D) All of the above will alter the equilibrium concentrations.
Q:
"If a stress is applied to a reaction mixture at equilibrium, the reaction occurs in the direction that will relieve the stress." This statement is called
A) the First Law of Thermodynamics.
B) the Law of Combining Volumes.
C) the Law of Mass Action.
D) Le Chtelier's principle.
Q:
Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: MaXb(s) a Mb+(aq) + b Xa-(aq). Given the following salts and their equilibrium constants for the reaction above at 25C, which salt is the least soluble?A) AgCl, Kc = 1.8 10-10B) Ag2SO4, Kc = 1.2 10-5C) CaCO3, Kc = 2.6 10-9D) CaF2, Kc = 1.5 10"10
Q:
The solubility of 1:1 salts is measured by the equilibrium constant for the general reaction: MX(s) = Mn+(aq) + Xn-(aq). Given the following salts and their equilibrium constants for the reaction above at 25C, which salt is the least soluble?
A) MgCO3, Kc = 6.8 10-6
B) CaCO3, Kc = 5.0 10-9
C) SrCO3, Kc = 5.6 10-10
D) BaCO3, Kc = 2.6 10-9
Q:
The equilibrium constant Kcfor the reaction HF(aq) + H2O(l) H3O+(aq) +F-(aq) is 3.5 10-4. What is the equilibrium concentration of H3O+ if the initial concentration of HF is 1.0 M?A) 1.0 MB) 3.5 10-2 MC) 1.9 10-2 MD) 1.9 10-4 M
Q:
For acid solutions of the same molarity acid strength is proportional to the equilibrium concentration of H3O+. For equimolar solutions of acids, which equilibrium expression below corresponds to the strongest acid?A) Kc = = 3.5 10-4B) Kc = = 3.5 10-8C) Kc = = 4.5 10-4D) Kc = = 4.9 10-10
Q:
Acids donate protons to water according to the general equation:HA(aq) + H2O(l) H3O+(aq) + A-(aq)Consider the following acids and their equilibrium constants for reaction with water at 25C. If all the acids have the same initial concentration, which is the strongest acid (i.e. which donates the most protons to water)?A) HBrO, Kc = 2.0 10-9B) HNO2, Kc = 4.5 10-4C) HF, Kc = 3.5 10-4D) HIO3, Kc = 1.7 10-1
Q:
Oxalic acid can donate two protons to water in successive reactions:(1) H2C2O4(aq) + H2O(l) H3O+(aq) + HC2O4-(aq)(2) HC2O4-(aq) + H2O(l) H3O+(aq) + C2O42-(aq)If Kc1 = 5.9 10-2 and Kc2 = 6.4 10-5 at 25C, what is the value of Kc for reaction (3)?(3) H2C2O4(aq) + 2 H2O(l) 2 H3O+(aq) + C2O42-(aq)A) 3.8 10-6B) 1.1 10-3C) 5.9 10-2D) 9.2 102
Q:
When reaction (1) and (2) below are added together, the result is reaction (3).1.H2O(l) + HNO2(aq) H3O+(aq) + NO2-(aq)2.H3O+(aq) + OH-(aq) 2 H2O(l)3.HNO2(aq) + OH-(aq) NO2-(aq) + H2O(l)If K1 = 4.50 10-4, and K2 = 1.00 1014, find the equilibrium constant, K3.A) 4.50 10-18B) 4.50 1010C) 1.00 1014D) 2.22 1017
Q:
Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: . At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr. What is the value of Kc at that temperature if the flask contains 0.104 mol of H2 at equilibrium?
A) 7.04 10-2
B) 4.40 10-2
C) 3.00 10-2
D) 2.10 10-1
Q:
Ammonium carbamate can dissociate into gases at 25C according to the reaction:NH2COONH4(s) 2 NH3(g) + CO2(g)If sufficient ammonium carbamate is sealed in a flask, the total pressure will be 0.117 atm at equilibrium. What is the value of Kp at 25C?A) 2.37 10-4B) 2.00 10-4C) 1.60 10-3D) 3.42 10-1
Q:
When baking soda is heated it decomposes according to the following reaction:2 NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g)If sufficient baking soda is placed in a container and heated to 90C, the total pressure of the gases is 0.5451 atm. What is the value of Kp at that temperature?A) 0.07428B) 0.2973C) 0.4228D) 1.091
Q:
Kp is equal to 48.70 at 731 K for the reaction: H2(g) + I2(g) 2 HI(g). Initially the mixture contains 0.08592 atm each of H2 and I2 and 1.0000 atm of HI. What is the pressure of HI at equilibrium?A) 0.7955 atmB) 0.9108 atmC) 0.9140 atmD) 0.9498 atm
Q:
The esterification of acetic acid and ethanol is given by the reaction below:C2H5OH(aq) + CH3COOH(aq) CH3COOC2H5(aq) + H2O(l)When 1.00 mol of ethanol was mixed with 2.00 mol of acid in a 1.00 L flask, 0.86 mol of ester was formed at room temperature. What is the value of the equilibrium constant, Kc?A) 0.43B) 2.3C) 4.6D) 5.4
Q:
Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: At 250C, 0.250 M PCl5 is added to a flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?
A) [PCl5] = 0.0280 M, [PCl3] = 0.222 M, [Cl2] = 0.222 M
B) [PCl5] = 1.25 M, [PCl3] = 0.474 M, [Cl2] = 0.474 M
C) [PCl5] = 1.80 M, [PCl3] = 1.80 M, [Cl2] = 1.80 M
D) [PCl5] = 2.27 M, [PCl3] = 2.02 M, [Cl2] = 2.02 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 0.125 atm of trans-2-butene, what is the equilibrium pressure of each gas?A) P(cis-2-butene) = 0.037 atm, P(trans-2-butene) = 0.125 atmB) P(cis-2-butene) = 0.048 atm, P(trans-2-butene) = 0.165 atmC) P(cis-2-butene) = 0.074 atm, P(trans-2-butene) = 0.250 atmD) P(cis-2-butene) = 0.085 atm, P(trans-2-butene) = 0.290 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) 0.23 MB) 0.28 MC) 0.45 MD) 0.56
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 0.100 M, respectively.A) [C6H12] = 0.0625 and [CH3C5H9] = 0.062 MB) [C6H12] = 0.138 and [CH3C5H9] = 0.162 MC) [C6H12] = 0.262 M and [CH3C5H9] = 0.038 MD) [C6H12] = 0.282 and [CH3C5H9] = 0.018 M
Q:
The following two isomers of C3H7NO exist in equilibrium with each other in solution: If Kc = 0.57 at 25C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M, what are the concentrations at equilibrium?
A) [reactant] = 0.43 M and [product] = 0.24 M
B) [reactant] = 0.67 M and [product] = 0.38 M
C) [reactant] = 0.76 M and [product] = 0.44 M
D) [reactant] = 0.82 M and [product] = 0.47 M
Q:
For the isomerization reaction:butane isobutaneKp equals 25 at 500C. If the initial pressures of butane and isobutane are 10. atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?A) P(butane) = 0.38 atm and P(isobutane) = 9.6 atmB) P(butane) = 0.40 atm and P(isobutane) = 10. atmC) P(butane) = 9.6 atm and P(isobutane) = 0.38 atmD) P(butane) = 10 atm and P(isobutane) = 0.40 atm
Q:
At a certain temperature, Kc equals 1.4 102 for the reaction:2 CO(g) + O2(g) 2 CO2(g).If a 2.50-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) 0.422 molB) 0.169 molC) 0.107 molD) 0.0114 mol
Q:
An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0015 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) 4.8 10-6 MB) 2.2 10-3 MC) 9.3 10-2 MD) 3.1 10-1 M
Q:
At a certain temperature, bromine and nitric oxide react to form nitrosyl bromide:Br2(g) + 2 NO(g) 2 NOBr(g). When 0.010 mol Br2 is mixed with 0.025 mol NO and 0.015 mol NOBr in a 2.50 L flask, the concentration of NOBr decreases. Which statement below is true?A) Kc < 36B) Kc > 36C) Kc < 90D) Kc > 90
Q:
At a certain temperature, bromine and nitric oxide react to form nitrosyl bromide:Br2(g) + 2 NO(g) 2 NOBr(g).When initial amounts of Br2, NO, and NOBr are mixed, the concentration of NOBr 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 the reaction will shift if the initial concentrations of C6H12 and MCP are 0.200 M and 0.100 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 1.00 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] = 1.20 M, [O2] = 0.45 M, and [SO3] = 1.80 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: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(l), the equilibrium constant is 0.063 at 400 K. If the reaction quotient is 0.100, which of the following statements is not correct?A) [HCl] will increase.B) [O2] will increase.C) [Cl2] will decrease.D) [H2O] will increase.
Q:
Which statement is true for a reaction with Kc equal to 2.43 10-12?
A) Increasing the temperature will not change the value of Kc.
B) There are appreciable concentrations of both reactants and products.
C) The reaction proceeds hardly at all towards completion.
D) The reaction proceeds nearly all the way to completion.
Q:
For the reaction, A(g) + 2 B(g) 2 C(g), Kc = 1 10-10 at 25C. Which of the following statements is true?A) n = +1B) The concentration of the products is greater than the concentration of the reactants.C) The reaction is favored in the reverse direction.D) The value of Kp will be larger than the value for Kc.
Q:
Given the hypothetical reaction: 2 A(s) + x B(g) 3 C(g), Kp = 0.0105 and Kc = 0.45 at 250C. What is the value of the coefficient x?A) 1B) 2C) 3D) 4
Q:
If Kc = 0.900, and Kp = 538 for a hypothetical reaction, which of the equations below could represent the reaction at 25C?A) A(g) + B(s) 3 C(g)B) A(l) + 2 B(g) 2 C(g)C) B(g) C(l) + D(l)D) A(g) 2 C(s) + D(g)
Q:
For which one of the following reactions will Kc = Kp?A) CO(g) + 2 H2(g) CH3OH(g)B) ZnO(s) + CO(g) Zn(s) + CO2(g)C) 2 O3(g) 3 O2(g)D) COCl2(g) CO(g) + Cl2(g)
Q:
What is the equilibrium constant, Kc, for the reaction: 2 Hg(l) + O2(g) 2 HgO(s) if the amounts of reactants and products at equilibrium are: 1.00 g of HgO(s), 2.00 mL of Hg(l), and 1.60 M O2(g)? (The molar mass and density of HgO(s) is 217 g/mol, and 1.10 g/cm3. The molar mass and density of Hg(l) is 201 g/mol, and 13.6 g/mL.)A) 6.85 10-4B) 4.66 10-2C) 0.625D) 1.46 103
Q:
What is the value for Kc for the following reaction:PbCl2(s) Pb2+(aq) + 2 Cl-(aq), if PbCl2(s) = 1.50 grams, [Pb2+] = 1.6 10-2 M and [Cl-] = 3.2 10-2 M at equilibrium? (The molar mass of PbCl2(s) is 278 g/mol and its density is 5.85 g/cm3.)A) 7.6 10-7B) 1.6 10-5C) 6.2 104D) 1.3 106
Q:
What is the equilibrium equation for the following reaction?2 H2O (l) H3O+ (aq) + OH" (aq)A) Kc = B) Kc = C) Kc = D) Kc = [H3O+] [OH"]
Q:
What is the equilibrium equation for the following reaction?FeS(s) + 2 H3O+ (aq) Fe2+(aq) + H2S (aq) + 2 H2O (l)A) Kc = B) Kc = C) Kc = D) Kc =
Q:
What is the equilibrium equation for the following reaction?C2H4 (g) + 3 O2 (g) 2 CO2 (g) + 2 H2O (l)A) Kp = B) Kp = C) Kp = D) Kp =
Q:
What is the equilibrium equation for the dissociation of formic acid in water?HCOOH (aq) + H2O (l) H3O+ (aq) + HCOO- (aq)A) Kc = B) Kc = C) Kc = D) Kc =
Q:
Which equilibrium below is homogeneous?A) BaSO4(s) Ba2+(aq) + SO42-(aq)B) 2 H2O2(l) 2 H2O(l) + O2(g)C) NH4NO3(s) N2O(g) + 2 H2O(g)D) 2 CO(g) + O2(g) 2 CO2(g)
Q:
As a rule, which of the following phases are not included in the equilibrium constant expression?
I. pure liquids II. pure solids III. aqueous solutions IV. gases
A) I, II
B) I, IV
C) III, IV
D) II, III
Q:
A 1.50 L vessel contains an equilibrium mixture of 0.100 mol of NO, 0.150 mol of Br2, and 0.250 mol of NOBr at 25C. What is the value of Kp for the reaction below?2 NO(g) + Br2(g) 2 NOBr(g)?A) 2.56B) 62.5C) 1.28 102D) 1.53 103
Q:
The decomposition of ammonia is: 2 NH3(g) N2(g) + 3 H2(g). If the pressure of ammonia is 1.0 10-3 atm, and the pressures of N2 and H2 are each 0.20 atm, what is the value for Kp' at 400C for the reverse reaction?A) -6.2 10-4B) -1.6 103C) 6.2 10-4D) 1.6 103
Q:
The decomposition of ammonia is: 2 NH3(g) N2(g) + 3 H2(g). If the partial pressure of ammonia is 1.6 10-3 atm and the partial pressures of N2 and H2 are each 0.25 atm at equilibrium, what is the value for Kc at 400C for the forward reaction?A) 0.50B) 1.4C) 1.5 103D) 4.6 106
Q:
The decomposition of ammonia is: 2 NH3(g) = N2(g) + 3 H2(g). If Kp is 1.5 103 at 400C, what is the partial pressure of ammonia at equilibrium when N2 is 0.10 atm and H2 is 0.15 atm?
A) 2.2 10-7 atm
B) 4.7 10-4 atm
C) 2.1 103 atm
D) 4.4 106 atm
Q:
Phosphorus pentachloride decomposes to phosphorus trichloride and chlorine gas at elevated temperatures by the following reaction:PCl5(g) PCl3(g) + Cl2(g). If Kc = 1.8 at 250C, what is the value of Kp at the same temperature?A) 4.2 10-2B) 8.8 10-2C) 65D) 77
Q:
If Kc = 2.0 x 1033 at 25C, for the following reaction: H2(g) + Cl2(g) 2 HCl(g), then find Kp at the same temperature.A) 8.2 1031B) 9.7 1032C) 2.0 1033D) 4.9 1034