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Chemistry
Q:
At a given temperature and pressure, which of the following would be expected to have the greatest molar entropy?
A) F2(s)
B) F2(l)
C) F2(g)
D) All of these would be expected to have the same molar entropy.
Q:
When 0.455 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a water jacket containing 500.0 g of water, the temperature of the water increases by 8.63C. Assuming that the specific heat of water is 4.18 J/(g C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene.A) +39.7 kJ/molB) -39.7 kJ/molC) -7070 kJ/molD) -8120 kJ/mol
Q:
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 23.0C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g C), calculate the final temperature of the solution.Ca2+(aq) + 2 F-(aq) -> CaF2(s) H = -11.5 kJA) 22.45CB) 23.55CC) 24.10CD) 24.65C
Q:
Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.0 25 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00C to 35.75C. If the specific heat of the solution is 4.18 J/(g C), calculate H for the reaction, as written.2 Na(s) + 2 H2O(l) -> 2 NaOH(aq) + H2(g) H= ?A) -5.41 kJB) -90.0 kJC) -180 kJD) -360 kJ
Q:
When 1.50 g of Ba(s) is added to 100.00 g of water in a container open to the atmosphere, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00C to 33.10C. If the specific heat of the solution is 4.18 J/(g C), calculate H for the reaction, as written.Ba(s) + 2 H2O(l) -> Ba(OH)2(aq) + H2(g) H = ?A) -431 kJB) -3.14 kJC) 3.14 kJD) 431 kJ
Q:
It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 23.0C to 68.0C. What is the specific heat of benzene?A) 1. 14 J/(g C)B) 1.72 J/(g C)C) 3.48 J/(g C)D) 5. 25 J/(g C)
Q:
The specific heat of copper is 0.385 J/(g C). If 34.2 g of copper, initially at 24.0C, absorbs4.689 kJ, what will be the final temperature of the copper?A) 24.4CB) 26.8CC) 356CD) 380C
Q:
Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 35.0C to gaseous CCl4 76.8C (the normal boiling point for CCl4)? The specific heat of CCl4(l) is0.857 J/(g C), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol.A) 0.896 kJB) 1.43 kJC) 5.74 kJD) 6.28 kJ
Q:
When 1.50 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 1062 kJ of heat are released. Calculate the value of H for this reaction, as written.2 CH4(g) + 3 Cl2(g) -> 2 CHCl3(l) + 3 H2(g) H = ?A) -1420 kJB) -708 kJC) +708 kJD) +1420 kJ
Q:
The heat of vaporization of water at 100C is 40.66 kJ/mol. Calculate the quantity of heat that is absorbed/released when 9.00 g of steam condenses to liquid water at 100C.
A) 20.3 kJ of heat are absorbed.
B) 20.3 kJ of heat are released.
C) 81.3 kJ of heat are absorbed.
D) 81.3 kJ of heat are released.
Q:
At constant pressure, the combustion of 15.0 g of C2H6(g) releases 777 kJ of heat. What is H for the reaction given below?2 C2H6(g) + 7 O2(g) -> 4 CO2(g) + 6 H2O(l)A) - 129 kJB) - 779 kJC) -1560 kJD) -3120 kJ
Q:
How much heat is absorbed when 45.00 g of C(s) reacts in the presence of excess SO2(g) to produce CS2(l) and CO(g) according to the following chemical equation?5 C(s) + 2 SO2(g) -> CS2(l) + 4 CO(g) H = 239.9 kJA) 179.8 kJB) 239.9 kJC) 898.5 kJD) 2158 kJ
Q:
How much heat is absorbed/released when 35.00 g of NH3(g) reacts in the presence of excess O2(g) to produce NO(g) and H2O(l) according to the following chemical equation?4 NH3(g) + 5 O2(g) -> 4 NO(g) + 6 H2O(l) H = 1168 kJA) 600.1 kJ of heat are absorbed.B) 600.1 kJ of heat are released.C) 2400 kJ of heat are absorbed.D) 2400 kJ of heat are released.
Q:
At 1 atm pressure, the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol. To the correct number of significant figures, how much heat is required to melt 2.50 mol of gallium at 1 atm pressure?
A) 6 kJ
B) 20 kJ
C) 262 kJ
D) 274 kJ
Q:
When 10.00 moles of H2(g) reacts with 5.000 mol of O2(g) to form 10.00 mol of H2O(l) at 25C and a constant pressure of 1.00 atm. If 683.0 kJ of heat are released during this reaction, and PV is equal to - 37.00 kJ, thenA) H = + 683.0 kJ and E = + 720.0 kJ.B) H = + 683.0 kJ and E = + 646.0 kJ.C)H = - 683.0 kJ and E = - 646.0 kJ.D) H = - 683.0 kJ and E = - 720.0 kJ.
Q:
When 5.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1C, 169.5 kJ are absorbed and PV for the vaporization process is equal to 14.5 kJ thenA) E = 155.0 kJ and H = 169.5 kJ.B) E = 184.0 kJ and H = 169.5 kJ.C) E = 169.5 kJ and H = 184.0 kJ.D) E = 169.5 kJ and H = 155.0 kJ.
Q:
For a particular process that is carried out at constant pressure, q = 145 kJ and w = - 35 kJ. Therefore,A) E = 110 kJ and H = 145 kJ.B) E = 145 kJ and H = 110 kJ.C) E = 145 kJ and H = 180 kJ.D) E = 180 kJ and H = 145 kJ.
Q:
Calculate the work, w, gained or lost by the system when a gas expands from 15 L to 40 L against a constant external pressure of 1.5 atm. 1 L atm = 101 JA) - 6.1 kJB) - 3.8 kJC) + 3.8 kJD) + 6.1 kJ
Q:
For a process at constant pressure, 49,600 calories of heat are released. This quantity of heat is equivalent to
A) 4.82 10- 6 J.
B) 1.19 104 J.
C) 1.24 104 J.
D) 2.08 105 J.
Q:
The following drawing is a representation of a reaction for which H = -22 kJ. This reaction is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and nonspontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
The following drawing is a representation of a reaction for which H = +62 kJ. This reaction is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and nonspontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
The following drawing is a representation of a reaction of the type A -> B, where different shaded spheres represent different molecular structures. For this reaction H = -30 kJ. This reaction is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and nonspontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
The following drawing is a representation of a reaction of the type A -> B, where different shaded spheres represent different molecular structures. For this reaction H = +45 kJ. This reaction is likely to beA) nonspontaneous at all temperatures.B) nonspontaneous at low temperatures and spontaneous at high temperatures.C) spontaneous at low temperatures and nonspontaneous at high temperatures.D) spontaneous at all temperatures.
Q:
This reaction is likely to be
A) nonspontaneous at all temperatures.
B) nonspontaneous at low temperatures and spontaneous at high temperatures.
C) spontaneous at low temperatures and nonspontaneous at high temperatures.
D) spontaneous at all temperatures.
Q:
What are the signs of H and S for this reaction?A) H = +, S = +B) H = +, S = -C) H = -, S = +D) H = -, S = -
Q:
The reaction represented in the above drawing is likely to be
A) nonspontaneous at all temperatures.
B) nonspontaneous at low temperatures and spontaneous at high temperatures.
C) spontaneous at low temperatures and non spontaneous at high temperatures.
D) spontaneous at all temperatures.
Q:
What are the signs of H and S for the reaction represented in the above drawing?A) H = +, S = +B) H = +, S = -C) H = -, S = +D) H = -, S = -
Q:
The reaction represented in the above drawing is likely to be
A) nonspontaneous at all temperatures.
B) nonspontaneous at low temperatures and spontaneous at high temperatures.
C) spontaneous at low temperatures and non spontaneous at high temperatures.
D) spontaneous at all temperatures.
Q:
What are the signs of H and S for the reaction represented in the above drawing?A) H = +,S = +B) H = +, S = -C) H = -, S = +D) H = -, S = -
Q:
Which atomic orbitals are involved in bonding and which as lone pair orbitals for N2H2? A) bonding: s on H, sp2 on N lone pair: p on N
B) bonding: sp2 on both H and N lone pair: p on N
C) bonding: s on H, p on N lone pair: sp2 on N
D) bonding: s on H, sp2 and p on N lone pair: sp2 on N
Q:
Which type of bond produces a charge cloud with a nodal plane containing the bond axis?A) B) C) and D) neither nor
Q:
The CO bond in COCl2 can be described as
A) a σ bond and a π bond, both involving sp hybrid orbitals on C.
B) a σ bond involving an sp hybrid orbital on C and a π bond involving a p orbital on C.
C) a σ bond and a π bond, both involving sp2 hybrid orbitals on C.
D) a σ bond involving an sp2 hybrid orbital on C and a π bond involving a p orbital on C.
Q:
Which of the following would be expected to have sp2 hybridization on atom A? A) II
B) I and III
C) I, II, and III
D) I and IV
Q:
What orbital hybridization is expected for the central atom in a molecule with a trigonal planar geometry?
A) sp
B) sp2
C) sp3
D) None of these
Q:
The orbital hybridization on the carbon atom in HCN is
A) sp.
B) sp2.
C) sp3.
D) None of these
Q:
A triple bond is generally composed ofA) three bonds.B) two bonds and one bond.C) one bond and two bonds.D) three bonds.
Q:
The number of sp2 hybrid orbitals on the carbon atom in CO32- isA) one.B) two.C) three.D) four.
Q:
Which of the following is not true?
A) The sp3 hybrid orbitals are degenerate.
B) An sp3 hybrid orbital may hold a lone pair of electrons.
C) An sp3 hybrid orbital may form a sigma bond by overlap with an orbital on another atom.
D) An sp3 hybrid orbital may form a pi bond by overlap with an orbital on another atom.
Q:
What is the angle between adjacent sp3 hybrid orbitals?
A) 90
B) 109.5
C) 120
D) 180
Q:
Which orbital hybridization is associated with a tetrahedral charge cloud arrangement?
A) sp
B) sp2
C) sp3
D) None of these
Q:
A single sp3 hybrid orbital has
A) one lobe.
B) two lobes of equal size.
C) two lobes of unequal size.
D) four lobes of equal size.
Q:
Which of the following is not a valence bond concept?
A) The greater the overlap between the orbitals on two atoms, the stronger the bond.
B) Lone pair electrons are in atomic orbitals or in hybrid atomic orbitals.
C) Atomic orbitals on two atoms may overlap to form antibonding orbitals.
D) A pair of electrons in a bond is shared by both atoms.
Q:
The VSEPR model predicts the OOO bond angle in O3 to be
A) 90.
B) 109.5.
C) less than 120 but greater than 109.5.
D) 120.
Q:
Arrange in order from the smallest to the largest bond angle: CH3+, NF3, NH4+, XeF4.
A) CH3+, NF3, NH4+, XeF4
B) NF3, NH4+, XeF4, CH3+
C) XeF4, NH4+, NF3, CH3+
D) XeF4, NF3, NH4+, CH3+
Q:
What is the smallest bond angle in SF6?
A) 60
B) 90
C) 109.5
D) 120
Q:
Which of the following best describes ICl2-? It has a molecular geometry that is
A) linear molecular shape with no lone pairs on the I atom.
B) linear molecular shape with lone pairs on the I atom.
C) non-linear molecular shape with no lone pairs on the I atom.
D) non-linear molecular shape with lone pairs on the I atom.
Q:
What is the molecular geometry of IF5?
A) octahedral
B) seesaw
C) square pyramidal
D) trigonal bipyramidal
Q:
What is the O-N-O bond angle in NO3-?
A) less than 109.5
B) 109.5
C) 120
D) greater than 120
Q:
What is the molecular geometry of AsCl3?
A) T-shaped
B) tetrahedral
C) trigonal planar
D) trigonal pyramidal
Q:
Which of the following should be nonlinear? A) only I
B) only II
C) only III
D) II and III
Q:
What is the molecular geometry of BrF4-?
A) seesaw
B) square planar
C) square pyramidal
D) tetrahedral
Q:
Which of the following should be nonplanar? A) only I
B) only II
C) only III
D) I and III
Q:
Based on VSEPR theory, which should have the smallest XAX bond angle?
A) B) C) D)
Q:
What geometric arrangement of charge clouds is expected for an atom that has five charge clouds?
A) tetrahedral
B) square planar
C) trigonal bipyramidal
D) octahedral
Q:
A molecular compound that obeys the octet rule in which all atoms have a zero formal charge is
A) BaCl2
B) BrF3
C) NCl3
D) XeF4
Q:
Based on formal charges, what is the SO bond order in SO42-?
A) 1
B) 1.3
C) 1.5
D) 2
Q:
How many double and single bonds are in the resonance form for SO2 in which the formal charges on each atom are zero?
A) two single bonds and no double bonds
B) one single bond and one double bond
C) no single bonds and two double bonds
D) Each of these is possible.
Q:
Assign formal charges to all atoms in the following resonance form for HNO3. A) 0 for all atoms
B) +1 for N, -1 for oxygen (c), 0 for all other atoms
C) +1 for N and H, -1 for oxygen (a) and oxygen (c), 0 for oxygen (b)
D) +1 for H, -2 for each oxygen, +5 for N
Q:
Which electron dot structure for OCN- has a formal charge of -1 on the most electronegative atom?
A) B) C) D)
Q:
Assign formal charges to each atom in the resonance form for SOCl2 given below. A) 0 for Cl, 0 for S, and 0 for O
B) 0 for Cl, +1 for S, and -1 for O
C) -1 for Cl, +4 for S, and -2 for O
D) -1 for Cl, -2 for S, and -2 for O
Q:
Assign formal charges to each atom in the resonance form for SOCl2 given below. A) 0 for Cl, 0 for S, and 0 for O
B) 0 for Cl, +1 for S, and -1 for O
C) -1 for Cl, +4 for S, and -2 for O
D) -1 for Cl, -2 for S, and -2 for O
Q:
Two resonance forms for SOCl2 are given below. Which is favored by the octet rule and which by formal charge considerations?
A) I is favored by the octet rule and by formal charge considerations.
B) I is favored by the octet rule and II by formal charge considerations.
C) II is favored by the octet rule and I by formal charge considerations.
D) II is favored by the octet rule and by formal charge considerations.
Q:
Based on formal charge considerations, the electron-dot structure of CO32" ion has
A) two resonance structures involving two single bonds and one double bond.
B) two resonance structures involving one single bond and two double bonds.
C) three resonance structures involving two single bonds and one double bond.
D) three resonance structures involving one single bond and two double bonds.
Q:
Which one of the following is expected to exhibit resonance?
A) NH4+
B) HCN
C) CO2
D) NO2-
Q:
Which of the following are allowed resonance forms of NCS-? A) only I
B) only II
C) only III
D) I and III
Q:
Which is expected to have the strongest CO bond?
A) CH3OH
B) COCl2
C) CH3CO2-
D) CO32-
Q:
What is the approximate carbon-oxygen bond order in CO32-?
A) 1
B) 4/3
C) 5/3
D) 2
Q:
How many resonance structures are required in the electron-dot structure of CO32-?
A) two
B) three
C) four
D) five
Q:
NO2- is be expected to haveA) two single bonds.B) one single and one double bond.C) two double bonds.D) two identical bonds intermediate between a single and a double bond.
Q:
How many lone pairs are on the Br atom in BrF2-?
A) 0
B) 1
C) 2
D) 3
Q:
Consider a molecule with the following connections: When a valid electron dot structure is written, how many double bonds will the molecule contain?
A) 0
B) 1
C) 2
D) 4
Q:
Identify the fourth-row element X that forms the ion. A) Ge
B) As
C) Se
D) Kr
Q:
How many electrons are in the valence shell of I in IF4-?
A) 8
B) 10
C) 12
D) 14
Q:
How many lone pairs of electrons are on the Xe atom in XeF6?
A) 0
B) 1
C) 2
D) 3
Q:
Which of the following contains an atom that does not obey the octet rule?
A) KBr
B) CO2
C) ClF3
D) ICl
Q:
Which element can accommodate more than eight electrons in its valence shell?
A) C
B) O
C) P
D) He
Q:
Elements that can accommodate more than eight electrons in their valence shell occur only in periodic table period
A) 2 or lower.
B) 3 or lower.
C) 4 or lower.
D) 5 or lower.
Q:
Which molecule contains a triple bond?
A) F2
B) O3
C) HCN
D) H2CO
Q:
In the most acceptable electron-dot structure for carbonyl fluoride, COF2 the central atom is
A) C, which is singly-bonded to O.
B) C, which is doubly-bonded to O.
C) O, which is singly-bonded to C
D) O, which is doubly-bonded to C.
Q:
Which is the most acceptable electron dot structure for N2H2?A)B)C)H - N N - HD)