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Chemistry
Q:
Given the following hypothetical reaction: 2 E(g) + F(g) + G(g) -> products. If the rate law is: Rate = k[E]2[F]-1, what is the order of reaction with respect to E?A) zeroB) firstC) secondD) third
Q:
The hydrolysis of tert-butyl chloride is given in the reaction below:(CH3)3CCl(aq) + H2O(l) -> (CH3)3COH(aq) + H+(aq) + Cl-(aq)If the rate law is: Rate = k[(CH3)3CCl], what is the order of the reaction with respect to water?A) zeroB) firstC) secondD) third
Q:
The reaction between chlorine and nitric oxide to form nitrosyl chloride is shown below. If the reaction rate doubles when the concentration of Cl2 is doubled and the rate quadruples when the concentration of NO is doubled, by what factor will the rate increase if both concentrations, NO and Cl2, are doubled?Cl2(g) + 2 NO(g) -> 2 NOCl(g)A) 2B) 4C) 8D) 16
Q:
For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of B is increased by a factor of 2.00? The rate will
A) decrease by a factor of 1/4.00.
B) decrease by a factor of 1/2.00.
C) increase by a factor of 2.00.
D) increase by a factor of 4.00.
Q:
For a reaction that follows the general rate law, Rate = k[A][B]2, what will happen to the rate of reaction if the concentration of A is increased by a factor of 3.00? The rate will
A) decrease by a factor of 1/9.00.
B) decrease by a factor of 1/3.00.
C) increase by a factor of 3.00.
D) increase by a factor of 9.00.
Q:
The reaction shown below has the rate law: Rate = k[BrO3-][Br-][H+]2.BrO3-(aq) + 5 Br-(aq) + 6 H+(aq) -> 3 Br2(aq) + 3 H2O(l)What is the overall order of reaction?A) firstB) secondC) thirdD) fourth
Q:
Which statement is true for the general rate law: Rate = k[A]m[B]n?
A) It can be written from the stoichiometry of the overall reaction.
B) The overall order of the reaction is equal to m times n.
C) The values for the exponents must be determined by experiment.
D) The exponents in the rate law must be positive integers.
Q:
A concentration-time study of the gas phase reaction 2 A3 -> 3 A2 produced the data in the table below.Time (s) [A3] (M) [A2] (M) 0 4.00 x 10-4 0 10 2.00 x 10-4 3.00 x 10-4 20 1.00 x 10-4 4.50 x 10-4 30 5.00 x 10-5 ?What is the concentration of A2 after 30 seconds?A) 5.00 10-4 MB) 5.25 10-4 MC) 5.50 10-4 MD) 6.00 10-4 M
Q:
A concentration-time study of the gas phase reaction 2 A3 -> 3 A2 produced the data in the table below. Time (s) [A3] (M) [A2] (M) 0 4.00 x 10-4 0 10 2.00 x 10-4 3.00 x 10-4 20 1.00 x 10-4 4.50 x 10-4 30 5.00 x 10-5 ?What is the average rate of formation of A2 in the time interval 20-30 seconds?A) 6.00 10-4 M/sB) 5.25 10-5 M/sC) 7.50 10-6 M/sD) 6.00 10-6 M/s
Q:
A concentration-time study of the gas phase reaction 2 A3 -> 3 A2 produced the data in the table below.Time (s) [A3] (M) [A2] (M) 0 4.00 x 10-4 0 10 2.00 x 10-4 3.00 x 10-4 20 1.00 x 10-4 4.50 x 10-4 30 5.00 x 10-5 ?What is the average rate of decomposition of A3 in the time interval 20-30 seconds?A) 4.00 10-4 M/sB) 3.50 10-5 M/sC) 5.00 10-6 M/sD) 4.00 10-6 M/s
Q:
Hydrogen peroxide decomposes to water and oxygen according to the reaction below:2 H2O2(aq) -> 2 H2O(l) + O2(g)In the presence of large excesses of I- ion, the following set of data is obtained. What is the average rate of disappearance of H2O2(aq) in M/s in the first 45.0 seconds of the reaction if 1.00 L of H2O2 reacts at 25C and 1.00 atm pressure?A) 9.09 10-7 M/sB) 3.63 10-6 M/sC) 4.33 10-5 M/sD) 1.64 10-4 M/s
Q:
The decomposition of dinitrogen pentoxide is described by the chemical equation2 N2O5(g) -> 4 NO2(g) + O2(g)If the rate of appearance of O2 is equal to 2.40 mol/min at a particular moment, what is the rate of disappearance of N2O5 at that moment?A) 0.600 mol/minB) 1.20 mol/minC) 4.80 mol/minD) 9.60 mol/min
Q:
The decomposition of dinitrogen pentoxide is described by the chemical equation2 N2O5(g) -> 4 NO2(g) + O2(g)If the rate of appearance of NO2 is equal to 0.560 mol/min at a particular moment, what is the rate of appearance of O2 at that moment?A) 0.140 mol/minB) 0.280 mol/minC) 1.12 mol/minD) 2.24 mol/min
Q:
The decomposition of dinitrogen pentoxide is described by the chemical equation2 N2O5(g) -> 4 NO2(g) + O2(g)If the rate of disappearance of N2O5 is equal to 1.40 mol/min at a particular moment, what is the rate of appearance of NO2 at that moment?A) 0.700 mol/minB) 1.40 mol/minC) 2.80 mol/minD) 5.60 mol/min
Q:
The reaction that occurs in a Breathalyzer, a device used to determine the alcohol level in a person's bloodstream, is given below. If the rate of appearance of Cr2(SO4)3 is 1.24 mol/min at a particular moment, what is the rate of disappearance of C2H6O at that moment?2 K2Cr2O7 + 8 H2SO4 + 3 C2H6O -> 2 Cr2(SO4)3 + 2 K2SO4 + 11 H2OA) 0.413 mol/minB) 0.826 mol/minC) 1.86 mol/minD) 3.72 mol/min
Q:
Hydroquinone, HOC6H6OH, can be formed by the reaction with acetylene below:2 HCCH + 3 CO + H2O -> HOC6H4OH + CO2How is the rate of disappearance of acetylene, HCCH, related to the appearance of hydroquinone (Hq)?- = ?A) + B) + C) + D) +
Q:
Methanol can be produced by the following reaction:CO(g) + 2 H2(g) -> CH3OH(g).How is the rate of disappearance of hydrogen gas related to the rate of appearance of methanol?- = ?A) + B) + C) + 2 D) none of these
Q:
The burning of propane can be represented by the following equation:(g) + 7(g) -> 3(g) + 4O(g)Which of the following relationships is true?A) = B) - 7 = + 4C) - 3 = + 7D) + 7 = - 4
Q:
The burning of propane can be represented by the following equation:(g) + 7(g) -> 3(g) + 4O(g)The general rate of this reaction may be expressed as:A) + B) - C) - D) +
Q:
Molecular hydrogen can be made from methane gas by the reaction below. How is the rate of disappearance of CH4 related to the rate of appearance of H2?- = ?CH4 (g) + H2O (l) -> CO (g) + 3H2 (g)A) + B) + C) + 3 D) none of these
Q:
"Instantaneous rate" is defined as the
A) change in concentration per unit time.
B) equation showing how the rate depends on the concentration of each reactant.
C) rate of reaction at a particular time.
D) rate of reaction during a time interval.
Q:
Which term describes the measure of the increase in the concentration of a product per unit time?
A) activation energy
B) kinetics
C) reaction rate
D) reaction time
Q:
Naproxen is a commercially important anti-inflammatory agent that can be isolated from the thyroid gland. A solution of 1.138 g of naproxen in 25.00 g benzene has an osmotic pressure of 4.00 atm at 20C. The density of benzene is 0.8787 g/mL at this temperature. Calculate the molar mass of naproxen, assuming it remains intact upon dissolution and the density of the solution equals the density of pure benzene.
A) 176 g/mol
B) 230 g/mol
C) 307 g/mol
D) 3.80 105 g/mol
Q:
The coolant in automobiles is often a 50/50 % by volume mixture of ethylene glycol, HOCH2CH2OH, and water. At 20C, the density of ethylene glycol is 1.1088 g/mL and the density of water is 0.9982 g/mL. Assuming that the volumes are additive, what is the expected freezing point of a 50/50(v/v)% ethylene glycol/water solution? Kf = 1.86C/m for water.
A) -16C
B) -17C
C) -30C
D) -33C
Q:
When ethylene glycol, HOCH2CH2OH, is added to the water in an automobile radiator, the effect is to
A) lower the boiling point and lower the freezing point.
B) lower the boiling point and raise the freezing point.
C) raise the boiling point and lower the freezing point.
D) raise the boiling point and raise the freezing point.
Q:
When 0.500 g of vitamin K is dissolved in 10.0 g of camphor (Kf = 40.0C/m), the freezing point of the solution is 4.43C lower than that of pure camphor. Assuming vitamin K is a nonelectrolyte in camphor, calculate its molar mass.
A) 0.451 g/mol
B) 55.4 g/mol
C) 451 g/mol
D) 3.54 104 g/mol
Q:
The average osmotic pressure of blood is about 7 atm. Therefore
A) the average blood pressure is about 7 atm.
B) the average pressure inside the body is about 7 atm above the external pressure.
C) a pressure of about 7 atm would be required to prevent osmosis if blood is in contact with pure water across a semipermeable membrane.
D) All of the above are true.
Q:
A solution is made by dissolving 13 g of sucrose, C12H22O11, in 117 g of water, producing a solution with a volume of 125 mL at 20C. What is the expected osmotic pressure at 20C?
A) 7.3 atm
B) 10 atm
C) 14 atm
D) 58 atm
Q:
Assuming that sea water is a 3.5 mass % solution of NaCl in water, calculate its osmotic pressure at 20C. The density of a 3.5% NaCl solution at 20C is 1.023 g/mL.
A) 1.0 atm
B) 15 atm
C) 29 atm
D) 100 atm
Q:
How will the osmotic pressure of an aqueous solution change as evaporation occurs?
A) The osmotic pressure will increase.
B) The osmotic pressure will not change.
C) The osmotic pressure will decrease.
D) The osmotic pressure will increase or decrease until it equals the vapor pressure of water.
Q:
Red blood cells are placed into pure water. Which of the following statements is true?
A) Water molecules flow out of the red blood cells, causing them to collapse.
B) Water flows into the red blood cells, causing them to swell and burst.
C) The osmotic pressure of the cell contents increases, causing the cells to burst.
D) The osmotic pressure inside the cells equals the osmotic pressure outside.
Q:
Two aqueous solutions, A and B, are separated by a semipermeable membrane. The osmotic pressure of solution A immediately begins to decrease. Which of the following statements is true?
A) Solvent molecules are moving from solution B into solution A.
B) The initial osmotic pressure of solution B is greater than that of solution A.
C) The solvent molecules are moving from the solution of higher osmotic pressure to that of lower osmotic pressure.
D) Both B and C are true statements.
Q:
Chloroform has a boiling point of 61.1C and dichloromethane has a boiling point of 40.0C. When 0.100 mol of dichloromethane is added to 0.900 mol of chloroform, the resulting solution will have a boiling point
A) between 40.0C and 61.1C, but closer to 61.1C.
B) between 40.0C and 61.1C, but closer to 40.0C.
C) greater than 61.1C.
D) less than 40.0C.
Q:
An aqueous CsCl solution is 8.00 mass % CsCl and has a density of 1.0643 g/mL at 20C. What is the boiling point of this solution? Kb = 0.51C/m for water.
A) 100.27C
B) 100.53C
C) 103.8C
D) 104.3C
Q:
A 0.51 m aqueous solution of an unknown solute has a boiling point elevation of 0.62C. The boiling point elevation of a 0.51 m solution of a nonionizing molecular solute in water is 0.26C. How many moles of particles are formed per mole of solute when the unknown solute is dissolved in water?
A) 1.4
B) 2.0
C) 2.4
D) 3.0
Q:
A solution of 0.2113 g of water dissolved in 25.0 g of a solvent freezes at 11.5C below the freezing point of the solvent. What is Kf for this solvent?
A) 0.735C/m
B) 1.36C/m
C) 5.39C/m
D) 24.5C/m
Q:
An aqueous solution has a normal boiling point of 102.0C. What is the freezing point of this solution? For water Kb is and A) -0.55C
B) -2.0C
C) -3.6C
D) -7.3C
Q:
The normal boiling point of pure benzene is found to be 80.10C. What is the approximate molecular weight of a nonionizing substance if a solution of 3.55 g of the substance dissolved in 100. g of benzene has a normal boiling point of for benzene, C6H6.
A) 20 amu
B) 500 amu
C) 2000 amu
D) 20,000 amu
Q:
What is the freezing point of a solution of 1.43 g MgCl2 in 100 g of water? Kf for water is 1.86C/m for water.
A) -0.0279C
B) -0.279C
C) -0.559C
D) -0.838C
Q:
Calculate the freezing point of a solution of 20.0 g methyl salicylate, C7H6O2, dissolved in 800. g of benzene, C6H6. Kf for benzene is and the freezing point is 5.50C for benzene.
A) -1.05C
B) 1.05C
C) 4.45C
D) 6.54C
Q:
What is the expected freezing point of a 0.50 m solution of Na2SO4 in water? Kf for water is 1.86C/m.
A) -0.93C
B) -1.9C
C) -2.8C
D) -6.5C
Q:
Which of the following pairs of solutions have roughly the same boiling point elevation?
A) 0.100 m C6H12O6 and 0.0333 m CuCl2
B) 0.100 m NaCl and 0.100 m C6H12O6
C) 0.200 m NaCl and 0.300 m Na2SO4
D) 0.100 m KCl and 0.0500 m MgBr2
Q:
Which of the following solutions will have the lowest freezing point?
A) 0.0100 m NaCl
B) 0.0100 m Li2SO4
C) 0.035 m CH3CH2CH2OH
D) 0.015 m MgCl2
Q:
A 0.020 m aqueous solution containing which solute will have the lowest freezing point?
A) LiCl
B) NaCl
C) KCl
D) All will have approximately the same freezing point.
Q:
A 0.50 m solution of which solute has the largest van't Hoff factor?
A) CaCl2
B) K3PO4
C) LiCO3
D) NaNO3
Q:
When 2.36 g of a nonvolatile solute is dissolved in 100 g of solvent, the largest change in freezing point will be achieved when the solvent is
A) benzene, Kf = 5.07.
B) camphor, Kf = 37.8.
C) chloroform, Kf = 4.70.
D) All are expected to have the same freezing point.
Q:
If one mole of each is dissolved in 1.00 L of water, which will lower the vapor pressure the most?
A) C12H22O11
B) NaNO3
C) C3H7OH
D) MgCl2
Q:
An aqueous solution has a normal boiling point of 102.0C. What is the freezing point of this solution? For water Kb is and A) -0.55C
B) -2.0C
C) -3.6C
D) -7.3C
Q:
The normal boiling point of pure benzene is found to be 80.10C. What is the approximate molecular weight of a nonionizing substance if a solution of 3.55 g of the substance dissolved in 100. g of benzene has a normal boiling point of for benzene, C6H6.
A) 20 amu
B) 500 amu
C) 2000 amu
D) 20,000 amu
Q:
What is the freezing point of a solution of 1.43 g MgCl2 in 100 g of water? Kf for water is 1.86C/m for water.
A) -0.0279C
B) -0.279C
C) -0.559C
D) -0.838C
Q:
Calculate the freezing point of a solution of 20.0 g methyl salicylate, C7H6O2, dissolved in 800. g of benzene, C6H6. Kf for benzene is and the freezing point is 5.50C for benzene.
A) -1.05C
B) 1.05C
C) 4.45C
D) 6.54C
Q:
What is the expected freezing point of a 0.50 m solution of Na2SO4 in water? Kf for water is 1.86C/m.
A) -0.93C
B) -1.9C
C) -2.8C
D) -6.5C
Q:
Which of the following pairs of solutions have roughly the same boiling point elevation?
A) 0.100 m C6H12O6 and 0.0333 m CuCl2
B) 0.100 m NaCl and 0.100 m C6H12O6
C) 0.200 m NaCl and 0.300 m Na2SO4
D) 0.100 m KCl and 0.0500 m MgBr2
Q:
Which of the following solutions will have the lowest freezing point?
A) 0.0100 m NaCl
B) 0.0100 m Li2SO4
C) 0.035 m CH3CH2CH2OH
D) 0.015 m MgCl2
Q:
A 0.020 m aqueous solution containing which solute will have the lowest freezing point?
A) LiCl
B) NaCl
C) KCl
D) All will have approximately the same freezing point.
Q:
A 0.50 m solution of which solute has the largest van't Hoff factor?
A) CaCl2
B) K3PO4
C) LiCO3
D) NaNO3
Q:
When 2.36 g of a nonvolatile solute is dissolved in 100 g of solvent, the largest change in freezing point will be achieved when the solvent is
A) benzene, Kf = 5.07.
B) camphor, Kf = 37.8.
C) chloroform, Kf = 4.70.
D) All are expected to have the same freezing point.
Q:
If one mole of each is dissolved in 1.00 L of water, which will lower the vapor pressure the most?
A) C12H22O11
B) NaNO3
C) C3H7OH
D) MgCl2
Q:
How many grams of sucrose, C12H22O11, must be added to 500. g of water at 100C to change the vapor pressure to 752 mm Hg?
A) 0.295 g
B) 5.32 g
C) 10.6 g
D) 101 g
Q:
At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the mole fraction of benzene in the vapor phase over a solution of benzene and toluene with Xbenzene = 0.600.
A) 0.600
B) 0.678
C) 0.756
D) 0.823
Q:
At a given temperature the vapor pressures of benzene and toluene are 183 mm Hg and 59.2 mm Hg, respectively. Calculate the total vapor pressure over a solution of benzene and toluene with Xbenzene = 0.600.
A) 110 mm Hg
B) 121 mm Hg
C) 133 mm Hg
D) 242 mm Hg
Q:
A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25C. What is the vapor pressure of the solution if the vapor pressure of water at 25C is 23.76 mm Hg?
A) 20.5 mm Hg
B) 22.1 mm Hg
C) 22.9 mm Hg
D) 25.5 mm Hg
Q:
Which of the following is not an application of colligative properties?
A) adding silver to mercury to lower the vapor pressure of mercury
B) desalinating sea water by reverse osmosis
C) melting snow by application of salt
D) reduced boiling points of pure liquids at increased altitudes
Q:
The solubility of argon in water at 25C is 0.0150 mol/L. What is the Henry's Law constant for argon if the partial pressure of argon in air is 0.00934 atm?
A) 1.40 10-4 mol/(L atm)
B) 0.623 mol/(L atm)
C) 1.61 mol/(L atm)
D) 4.10 mol/(L atm)
Q:
The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L atm) at 25C. What is the solubility of methyl bromide in water at 25C and at a partial pressure of 250. mm Hg?
A) 0.0523 mol/L
B) 0.329 mol/L
C) 0.483 mol/L
D) 39.8 mol/L
Q:
In which case should CO2(g) be more soluble in water?
A) The total pressure is 5 atm and the partial pressure of CO2 is 1 atm.
B) The total pressure is 3 atm and the partial pressure of CO2 is 2 atm.
C) The total pressure is 1 atm and the partial pressure of CO2 is 0.03 atm.
D) The total pressure is 1 atm and the partial pressure of CO2 is 0.5 atm.
Q:
The solubility of gaseous solutes in liquid solvents is greater when the
A) external pressure over the solution is increased.
B) external pressure is decreased.
C) partial pressure of the gas above the solution is increased.
D) partial pressure of the solvent is increased.
Q:
In general, as the temperature increases, the solubility of gases in water ________ and the solubility of most solids in water ________.
A) decreases, decreases
B) decreases, increases
C) increases, decreases
D) increases, increases
Q:
Which of the following statements is true for a supersaturated solution?
A) The solute in the solution is at equilibrium with undissolved solute.
B) The solution contains more than the equilibrium amount of solute.
C) The solution is stable and the solute will not precipitate.
D) A supersaturated solution is more than 50% solute by mass.
Q:
Which of the following does not affect the solubility of a solute in a given solvent?
A) polarity of the solute
B) polarity of the solvent
C) rate of stirring
D) temperature of the solvent and solute
Q:
A saturated solution is defined as
A) a concentrated solution.
B) a solution that is in equilibrium with pure solvent.
C) a solution than is in equilibrium with undissolved solute.
D) a solution that is in equilibrium with both pure solvent and undissolved solute.
Q:
At 25.0C, a solution has a concentration of 3.179 M and a density of 1.260 g/mL. The density of the solution at 50.0C is 1.249 g/mL. What is the molarity of the solution at 50.0C?
A) 2.545 M
B) 3.151 M
C) 3.179 M
D) 3.230 M
Q:
A solution of LiCl in water is 18.0 mass % LiCl. What is the mole fraction of LiCl?
A) 0.0853
B) 0.0933
C) 0.425
D) 4.56
Q:
A solution of LiCl in water has XLiCl = 0.0500. What is the molality?
A) 2.60 m LiCl
B) 2.77 m LiCl
C) 2.92 m LiCl
D) 5.26 m LiCl
Q:
A 2.00 M solution of CaCl2 in water has a density of 1.17 g/mL. What is the mole fraction of CaCl2?
A) 0.0348
B) 0.0360
C) 0.0366
D) 0.0380
Q:
A 3.17 m solution of CaCl2 in water has a density of 1.24 g/mL. What is the molarity?
A) 2.56 M CaCl2
B) 2.91 M CaCl2
C) 3.50 M CaCl2
D) 3.93 M CaCl2
Q:
A 1.30 M solution of CaCl2 in water has a density of 1.11 g/mL. What is the molality?
A) 1.17 m CaCl2
B) 1.25 m CaCl2
C) 1.35 m CaCl2
D) 1.44 m CaCl2
Q:
Sodium hydroxide is available commercially as a 50.0% by weight aqueous solution. Calculate the molality of this sodium hydroxide solution.
A) 0.450 m
B) 19.1 m
C) 25.0 m
D) 125. m
Q:
Sodium hydroxide is available commercially as a 50.0% by weight aqueous solution. The density of the solution is 1.53 g/mL. Calculate the molarity of this sodium hydroxide solution.
A) 0.450 M
B) 19.1 M
C) 25.0 M
D) 125. M
Q:
Aqueous solutions of 30.0% (by mass) hydrogen peroxide, H2O2, are used to oxidize metals or organic molecules in chemical reactions. Calculate the molality of this solution.
A) 0.974 m
B) 6.78 m
C) 9.79 m
D) 12.6 m