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WorksheetsAP CHEM REVIEW QUIZ 2
Total questions: 25
Worksheet time: 50mins
The rate law for the reaction represented by the equation shown here is Rate = k[NO2][F2]. Which of the following could be the first elementary step of a two step mechanism if the first step is slow and the second step is fast?
F2(g) --> 2F(g)
NO2(g) + F2(g) --> NO2F(g) + F(g)
NO2(g) + F(g) --> NO2F(g)
2NO2(g) + F2(g) --> 2NO2F(g)
Which molecule has the smallest bond angle?
CH4
NH3
H2O
CO2
A mixture containing equal numbers of moles of ethyl acetate was separated using distillation. Based on the diagrams shown above, which of the following identifies the substance that would be initially present in higher concentration in the distillate and correctly explains why that matters?
Ethyl acetate, because it has fewer C - C bonds to break.
Ethyl acetate, because it has a shorter carbon chain and weaker London dispersion forces.
Butyl acetate, because it has more C - C bonds to break.
Butyl acetate, because it has a longer carbon chain and weaker dipole-dipole attractions.
A certain reaction: A(aq) + B(aq) <===> C(aq)
is studied. A is blue, B is colorless, and C is yellow. The reaction is 0-order with respect to [B]. A 5.0 mL sample of 0.001 Molar A is added to a 5.0 mL sample of 0.40 Molar B and mixed thoroughly. 1 mL of this mixture is added to a cuvette which is then placed in a spectrophotometer. The reaction progress is documented. The following results were obtained.
Approximately how much time was needed for 75% of the initial amount of A to react?
10s
30s
60s
80s
A certain reaction: A(aq) + B(aq) <===> C(aq)
is studied. A is blue, B is colorless, and C is yellow. The reaction is 0-order with respect to [B]. A 5.0 mL sample of 0.001 Molar A is added to a 5.0 mL sample of 0.40 Molar B and mixed thoroughly. 1 mL of this mixture is added to a cuvette which is then placed in a spectrophotometer. The reaction progress is documented. The following results were obtained.
How would the initial rate of reaction change if the solution of A were diluted by a factor of 3 before being added to the solution of B?
The rate would not be affected
the rate would increase
the rate would decrease
the rate would decrease only if the solution of B were also diluted before being mixed with A.
CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) Kp = 7.7 x 1024 at 298 K
4 moles gaseous methane and 4 moles gaseous water are added to a previously evacuated rigid container. The mixture is sparked and allowed to react according to the equation above. At 298K, which of the following is true at equilibrium?
[CH4] =[H2O] = [CO] and [H2]>[CO]
[CH4] =[H2O] = [CO] and [H2] < [CO]
[H2] > [CO] > [CH4]
[CH4] =[H2O] and [H2] < [CO]
A 10.0 L container has a [CuNO3] = 2x10-4 Molar and a [Pb(NO3)2] = 1x10-2 molar. 9x10-3 moles NaBr is added to the container, according to the data in the table above, what will happen?
only PbBr2 will precipitate
only CuBr will precipitate
both PbBr2 and CuBr will precipitate
neither PbBr2 or CuBr will precipitate
The pH of a 0.01 M HCN solution (Ka = 6 x 10-10) would be approximately
1-2
3-4
5-6
6-7
The photoelectron spectra for Fluorine and neon are shown above. Which of the following answers provides the correct set of peaks for fluorine, and correct justification?
The solid line peaks represent fluorine. This is true because the solid peaks are slightly to the left of the dashed peaks and fluorine is to the left of neon in the periodic table
The solid line peaks represent fluorine. This is true because fluorine has fewer protons than neon.
The dashed line peaks represent fluorine. This is true because neon’s 3p sublevel has 6 electrons, whereas fluorine’s 3p sublevel has only 5 electrons, as shown on the peaks at approximately 4 MJ/mol
The dashed line peaks represent fluorine. This is true because neon has more protons than fluorine.
A rigid 10.0 L container holds neon gas at a very high pressure. The measured pressure is much larger than the pressure predicted by the ideal gas law. Which of the following is the best explanation for this?
neon atoms break into two boron atoms at high pressure
at high pressure, neon atoms are very attracted to one another, causing the atoms to hit the walls of their container less often than if they were not attracted to one another
the volume of the neon atoms is too large a fraction of the volume of the container to be negligible
none of the above
Two trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial, 1.2 g graphite reacts with 4.0 grams MgO (molar mass 40.). In the second trial, 1.2 g graphite reacts with 8.0 g MgO. In both trials, the same mass of magnesium is produced. Which of the following shows the correct limiting reactant and the correct amount of heat needed for the reaction?
Limiting Reactant = C; Heat required = 49kJ
Limiting Reactant = C; Heat required = 98kJ
Limiting Reactant = MgO; Heat required = 49kJ
Limiting Reactant = MgO; Heat required = 298kJ
Two trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial, 1.2 g graphite reacts with 4.0 grams MgO (molar mass 40.). In the second trial, 1.2 g graphite reacts with 8.0 g MgO.
Which of the following statements about the thermodynamic favorability at 25oC about the reaction is correct?
The reaction is not thermodynamically favorable
The reaction is thermodynamically favorable and is driven by the entropy change only
The reaction is thermodynamically favorable and is driven by the enthalpy change only
The reaction is thermodynamically favorable and is driven by both enthalpy and entropy changes.
Two trials for the reaction above are carried out, and the heat flow is measured using a calorimeter. In the first trial, 2.4 grams Mg reacts with 3.2 grams O2. In the second trial, 2.4 g Mg reacts with 6.4 g O2. In both trials, the same mass of magnesium oxide is produced. Which of the following shows the correct limiting reactant and the correct amount of heat produced by the reaction?
Limiting reactant = Mg; Heat produced = 60.kJ
Limiting reactant = Mg; Heat produced = 120.kJ
Limiting reactant = O2; Heat produced = 60.kJ
Limiting reactant = O2; Heat produced = 120.kJ
Atoms or ions of which element are reduced in the reaction above?
Cr: each ion gains 3 electrons
Na: each ion gains 1 electron
Br: each atom gains 1 electron
H: each ion gains 1 electron
2 H2(g) + O2(g) ---> 2 H2O (g)
What will the drawing of the energy vs. reaction coordinate diagram look like for the above reaction?
The reactants will be 520 kJ higher than the products
The reactants will be 520 kJ lower than the products
The reactants will be 420 kJ higher than the products
The reactants will be 420 kJ lower than the products
Based on the information in the table above, what would the most likely formula be for the unknown substance with chlorine?
XCl
XCl2
XCl3
X2Cl
2 NO(g) + Cl2(g) <===> 2 NOCl (g) Kp = 2 x 103 at 25oC
Samples of each of the above chemicals are added to a 10. L previously evacuated rigid container at 25oC until each has a partial pressure of 0.1 atm. The molecules are allowed to react until equilibrium is attained. At equilibrium, which species will have the highest pressure?
only NO
only Cl2
NOCl
both NO and Cl2
A pure solid substance is heated at 2.0 atm, forming liquid and then vapor. Which of the following correctly assigns the sign for the change in enthalpy and entropy for the process when moving from point X to point Y?
ΔHo = Positive ; ΔSo = Positive
ΔHo = Negative; ΔSo = Negative
ΔHo = Positive; ΔSo = Negative
ΔHo = Negative;ΔSo = Positive
N2(g) + 3 H2(g) <===> 2 NH3 (g)
ΔHo = -92 kJ/molrxn and Kp = 5 x 105 at 298 K.
Nitrogen and hydrogen gases are added to a previously evacuated 10.0 L rigid insulated container at 25oC to obtain initial partial pressures of 1.0 atm each. They are allowed to react until equilibrium is reached.
How will the temperature inside the container be affected as the reaction proceeds?
the temperature will steadily increase until equilibrium is achieved because the reaction is exothermic
the temperature will steadily decrease until equilibrium is achieved because the reaction is endothermic
the temperature will first increase, then because the total number of gas particles decreases, the temperature will decrease according to PV=nRT.
the temperature will first decrease, then slowly increase until equilibrium is achieved
N2(g) + 3 H2(g) <===> 2 NH3 (g)
ΔHo = -92 kJ/molrxn and Kp = 5 x 105 at 298 K.
Nitrogen and hydrogen gases are added to a previously evacuated 10.0 L rigid insulated container at 25oC to obtain initial partial pressures of 1.0 atm each. They are allowed to react until equilibrium is reached.
What can you conclude about the sign of ΔSo?
ΔSo must be greater than zero because Δngas= -2
ΔSo must be greater than zero because K > 1
ΔSo must be less than zero because Δngas = -2
ΔSo must be less than zero because K > 1
2 NO(g) + Cl2(g) <==> 2 NOCl (g)
ΔHo = -80 kJ/molRXN Kp = 2 x 103 at 25oC
Nitrogen monoxide and chlorine gases are added to a previously evacuated 10.0 L rigid insulated container at 25oC to obtain initial partial pressures of 1.0 atm each. They are allowed to react until equilibrium is reached.
How will the temperature inside the container be affected as the reaction proceeds?
the temperature will steadily increase until equilibrium is achieved because the reaction is exothermic
the temperature will steadily decrease until equilibrium is achieved because the reaction is endothermic
the temperature will first increase, then because the total number of gas particles decreases, the temperature will decrease according to PV=nRT.
the temperature will first decrease, then slowly increase until equilibrium is achieved
2 NO(g) + Cl2(g) <==> 2 NOCl (g)
ΔHo = -80 kJ/molRXN Kp = 2 x 103 at 25oC
Nitrogen monoxide and chlorine gases are added to a previously evacuated 10.0 L rigid insulated container at 25oC to obtain initial partial pressures of 1.0 atm each. They are allowed to react until equilibrium is reached.
What can you conclude about the sign of ΔSo?
ΔSo must be greater than zero because Δngas= -1
ΔSo must be greater than zero because K > 1
ΔSo must be less than zero because Δngas = -1
ΔSo must be less than zero because K > 1
Which of the following ranks the 3 bases above from weakest to strongest base?
C < B < A
A < B < C
A < C < B
B < C < A
Based on the information above and periodic trends, which of the following is the best hypothesis regarding the oxide(s)formed by Rb?
Rb will form only Rb2O
Rb will form only RbO2
Rb will form only Rb2O and Rb2O2
Rb will form only Rb2O, Rb2O2 and RbO2
3 AgNO3(aq) + Al(s) ---> Al(NO3)3(aq) + 3 Ag(s)
If 100. mL of 0.40 M AgNO3 is added to 0.270 g Al and allowed to react completely, which of the following is/are true?
aluminum is the limiting reactant and 0.030 moles silver nitrate remain
aluminum is the limiting reactant and 0.020 moles silver nitrate remain
0.040 moles silver are produced
0.030 moles silver are produced
