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Chemistry
Q:
Given: 4 NO2(g) + O2(g) -> 2 N2O5(g) H = -110.2 kJfind H for N2O5(g) -> 2 NO2(g) + 1/2 O2(g).A) -220.4 kJB) -55.1 kJC) 55.1 kJD) 220.4 kJ
Q:
Find H for the reaction C3H8(g) + 5 O2(g) -> 3 CO2(g) + 4 H2O(l).H = -2046 kJ for the reaction: C3H8(g) + 5 O2(g) -> 3 CO2(g) + 4 H2O(g), and the heat of vaporization of water is 44.0 kJ/mol. Note that H2O is a liquid in the first reaction and a gas in the second.A) -2222 kJB) -2090 kJC) -2002 kJD) -1870 kJ
Q:
Given: S (s) + O2 (g) -> SO2 (g) H = -296.1 kJ2 SO3 (g) -> 2 SO2 (g) + O2 (g) H = 198.2 kJFind H for : 2 S(s) + 3 O2(g) -> 2 SO3(g)A) -790.4 kJB) -394.0 kJC) -97.9 kJD) +97.9 kJ
Q:
When 0.455 g of anthracene, C14H10, is combusted in a bomb calorimeter that has a water jacket containing 500. 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 25.00C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of calculate the final temperature of the solution.Ca2+(aq) + 2 F-(aq) -> CaF2(s) H = -11.5 kJA) 24.45CB) 25.55CC) 26.10CD) 26.65C
Q:
Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide according to the chemical equation shown below. When 0.0300 mol of Na is added to 100.00 g of water, the temperature of the resulting solution rises from 25.00C to 37.90C. 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) -364 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 calculate 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:
Water has an unusually highA) electrical conductivity.B) heat of combustion.C) heat of formation.D) specific heat.
Q:
It takes 11.2 kJ of energy to raise the temperature of 145 g of benzene from 25.0C to 70.0C. What is the specific heat of benzene?A) 1.10 J/(g C)B) 1.72 J/(g C)C) 3.48 J/(g C)D) 5.41 J/(g C)
Q:
The specific heat of copper is 0.385 J/(g C). If 34.2 g of copper, initially at 25C, absorbs 4.689 kJ, what will be the final temperature of the copper?A) 25.4CB) 27.8CC) 356CD) 381C
Q:
10.0 g of a metal, initially at 25C, are placed into 10.0 g of water, initially at 100C. Which metal will have the highest final temperature? Shown after each metal is its specific heat in J/(gC).A) aluminum (0.902)B) copper (0.385)C) gold (0.129)D) iron (0.450)
Q:
Calculate the total quantity of heat required to convert 25.0 g of liquid CCl4(l) from 25.0C to gaseous CCl4 at 76.8C (the normal boiling point for CCl4)? The specific heat of CCl4(l) is its heat of fusion is and its heat of vaporization is A) 1.11 kJB) 1.64 kJC) 5.96 kJD) 6.49 kJ
Q:
When 0.250 mol of CH4(g) reacts with excess Cl2(g) at constant pressure according to the chemical equation shown below, 177 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 5.00 g of steam condenses to liquid water at 100C.
A) 11.3 kJ of heat are absorbed.
B) 11.3 kJ of heat are released.
C) 147 kJ of heat are absorbed.
D) 147 kJ of heat are released.
Q:
At constant pressure, the combustion of 5.00 g of C2H6(g) releases 259 kJ of heat. What is H for the reaction given below?2 C2H6(g) + 7 O2(g) -> 4 CO2(g) + 6 H2O(l).A) -43.2 kJB) -779 kJC) -1560 kJD) -3108 kJ
Q:
How much heat is absorbed when 30.00 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) 119.9 kJB) 239.9 kJC) 599.2 kJD) 1439 kJ
Q:
How much heat is absorbed/released when 20.00 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) 342.9 kJ of heat are absorbed.B) 342.9 kJ of heat are released.C) 1372 kJ of heat are absorbed.D) 1372 kJ of heat are released.
Q:
How much heat is transferred per mole of NH3(g) formed in the reaction shown below?N2(g) + 3 H2(g) ->2 NH3(g) H = - 92.2 kJA) 92.2 kJB) 46.1 kJC) 30.7 kJD) 15.4 kJ
Q:
At 1 atm pressure the heat of sublimation of gallium is 277 kJ/mol and the heat of vaporization is 271 kJ/mol. How much heat is required to melt 1.50 mol of gallium at 1 atm pressure?
A) 6 kJ
B) 9 kJ
C) 268 kJ
D) 271 kJ
Q:
At 25C the heat of fusion of aluminum is 10.6 kJ/mol and the heat of sublimation is 326.4 kJ/mol. What is the heat of vaporization of aluminum at 25C?
A) 158.2 kJ/mol
B) 168.5 kJ/mol
C) 315.8 kJ/mol
D) 337.0 kJ/mol
Q:
Which is the most exothermic reaction?A) CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(g)B) CH4(g) + 2 O2(g) -> CO2(g) + 2 H2O(l)C) CO2(g) + 2 H2O(l) -> CH4(g) + 2 O2(g)D) CO2(g) + 2 H2O(g) -> CH4(g) + 2 O2(g)
Q:
For the reaction I2(g) → I2(s), H = -62.4 kJ at 25C. Based on these data, at 25CA) Hvap = -62.4 kJ/mol.B) Hvap = 62.4 kJ/mol.C) Hsub = -62.4 kJ/mol.D) Hsub = 62.4 kJ/mol.
Q:
The enthalpy of fusion, or heat of fusion (Hfusion), of water is positive and corresponds to which physical change?A) H2O(g) -> H2O(s)B) H2O(l) -> H2O(s)C) H2O(s) -> H2O(l)D) H2O(s) -> H2O(g)
Q:
When 2.000 moles of H2(g) reacts with 1.000 mol of O2(g) to form 2.000 mol of H2O(l) at 25C and a constant pressure of 1.00 atm. If 136.6 kJ of heat are released during this reaction, and PV is equal to -7.400 kJ, thenA) H = +136.6 kJ and E = +144.0 kJ.B) H = +136.6 kJ and E = +129.2 kJ.C) H = -136.6 kJ and E = -129.2 kJ.D) H = -136.6 kJ and E = -144.0 kJ.
Q:
For an explosion in an open vessel, one would expectA) H to be positive and E to be less than H.B) H to be positive and E to be greater than H.C) H to be negative and E to be less than H.D) H to be negative and E to be greater than H.
Q:
When 1.00 mol of benzene is vaporized at a constant pressure of 1.00 atm and at its normal boiling point of 80.1C, 33.9 kJ are absorbed and PV for the vaporization process is equal to 2.90 kJ, thenA) E = 31.0 kJ and H = 33.9 kJ.B) E = 36.8 kJ and H = 33.9 kJ.C) E = 33.9 kJ and H = 31.0 kJ.D) E = 33.9 kJ and H = 36.8 kJ.
Q:
Find E for the reaction below if the process is carried out at a constant pressure of 1.00 atm and V (the volume change) = -24.5 L. (1 L atm = 101 J)2 CO(g) + O2 (g) -> 2 CO2(g) H = -566. kJA) +2.47 kJB) -2.47 kJC) -564 kJD) -568 kJ
Q:
Under thermodynamic standard state conditions the element oxygen occurs as
A) O(g)
B) O2(g)
C) O2(l)
D) O3(g)
Q:
At constant pressure for which of the reactions shown below should ΔH be greater than E ?I. 2 SO2(g) + O2(g) -> 2 SO3(g)II. C3H8(g) + 5 O2(g) -> 3 CO2(g) + 4 H2O(l)III. H2(g) + Cl2(g) -> 2 HCl(g)IV. N2O4(g) -> 2 NO2(g)A) I.B) III.C) IV.D) II. and IV.
Q:
For the reaction shown below, at constant pressure what can be said about PV and E?N2(g) + 3 H2(g) -> 2 NH3(g) H = - 92.2 kJA) PV > 0 and E > - 92.2 kJB) PV > 0 and E < - 92.2 kJC) PV < 0 and E > - 92.2 kJD) PV < 0 and E < - 92.2 kJ
Q:
A process is carried out at constant pressure. Given that 0 > H > E,A) the system absorbs heat and expands during the process.B) the system absorbs heat and contracts during the process.C) the system loses heat and expands during the process.D) the system loses heat and contracts during the process.
Q:
A process is carried out at constant pressure. Given that E is positive and H is negative,A) the system absorbs heat and expands during the process.B) the system absorbs heat and contracts during the process.C) the system loses heat and expands during the process.D) the system loses heat and contracts during the process.
Q:
For most chemical reactionsA) H is much larger than E.B) E is much larger than H.C) H is equal to E.D) the difference between H and E is very small.
Q:
For a particular process that is carried out at constant pressure, q = 125 kJ and w = -15 kJ. Therefore,A) E = 110 kJ and H = 125 kJ.B) E = 125 kJ and H = 110 kJ.C) E = 125 kJ and H = 140 kJ.D) E = 140 kJ and H = 125 kJ.
Q:
Most chemical reactions are carried out in one of two ways:I. in an open vessel at constant atmospheric pressureII. in a closed vesselWhich is true?A) H = q for condition I and E = q for condition IIB) E = q for condition I and H = q for condition IIC) H = w for condition I and E = w for condition IID) E = w for condition I and H = w for condition II
Q:
For a process at constant pressure,A) E = w and q = 0.B) E = q and w = 0.C) E = H.D) H = q.
Q:
For a process at constant volume,A) q = 0, w = 0, and E = 0.B) w = 0 and E = q.C) w = 0 and H = q.D) w = 0 and E = H.
Q:
Which depends only on the initial and final state?
A) q
B) w
C) q + w
D) q - w
Q:
An ideal gas expands into a vacuum (external pressure = 0) without gaining or losing heat. For this expansionA) E increases.B) E does not change.C) E decreases.D) E = TS
Q:
What is expected when the reaction shown below takes place in a thermally-insulated container outfitted with a movable piston at a constant atmospheric pressure of 1 atm?2 C2H6(g) + 7 O2(g) -> 4 CO2(g) + 6 H2O(g)A) Volume will decrease and work will be done by the system.B) Volume will decrease and work will be done on the system.C) Volume will increase and work will be done by the system.D) Volume will increase and work will be done on the system.
Q:
Calculate the work energy, w, gained or lost by the system when a gas expands from 15 L to 35 L against a constant external pressure of 1.5 atm. [1 L atm = 101 J]A) -5.3 kJB) -3.0 kJC) +3.0 kJD) +5.3 kJ
Q:
In which case is the work done on the system always positive?A) E > 0B) V > 0C) V = 0D) V < 0
Q:
Which is a measure of the sum of the kinetic and potential energies of each particle in the system?
A) E, the internal energy
B) G, the Gibbs free energy
C) H, the enthalpy
D) T, the temperature
Q:
The first law of thermodynamics
A) defines chemical energy.
B) defines entropy.
C) is a statement of conservation of energy.
D) provides a criterion for the spontaneity of a reaction.
Q:
Which of the following is not a state function?
A) altitude
B) heat
C) internal energy
D) volume
Q:
Which of the following is not a type of energy or energy transfer?
A) chemical energy
B) heat
C) pressure
D) work
Q:
At 298 K the average kinetic energy is the same for H2, He, and N2. The gas with the highest average velocity is
A) H2.
B) He.
C) N2.
D) All have the same average velocity.
Q:
A spontaneous reaction has a ________ value of G and is favored by a ________ value of H and a ________ value of ΔS.
Q:
When 1.0 mole of MgSO4 is dissolved in water contained in a calorimeter, the temperature of the water and dissolved ions increases. Therefore the sign of H for this reaction is ________, heat is transferred ________ the system ________ the surroundings, and the reaction is classified as ________.
Q:
Because the number of moles of gas are increasing from 6 to 7 in the reaction shown below, at constant pressure E is predicted to be slightly ________ negative than H.C3H8(g) + 5 O2(g) -> 3 CO2(g) + 4 H2O(g)
Q:
In the reaction shown below, ________ kJ of heat are released per mole of O2(g) that reacts.C3H8(g) + 5 O2(g) -> 3 CO2(g) + 4 H2O(g) H = - 2045 kJ
Q:
Heat transferred in a chemical reaction or physical change is expressed as E when the heat is transferred under constant ________ and is expressed as H when heat is transferred under constant ________ conditions.
Q:
A reaction for which E = - 450 kJ is one in which products have 450 kJ ________ internal energy than the reactants, and products are ________ stable than the reactants.
Q:
________ energy is the kinetic energy of molecular motion.
Q:
The SI unit for energy is the ________.
Q:
Kinetic energy increases with increasing ________ and increasing ________.
Q:
Energy can be classified as either ________ energy (energy of motion) or ________ energy (stored energy).
Q:
For the freezing of liquid bromine, Br2, at a given temperature and pressure,A) H is negative and S is negative.B) H is negative and S is positive.C)H is positive and S is negative.D) H is positive and S is positive.
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:
Calculate the heat of formation for CaC(s) given that ΔH for the following reaction is +178 kJ/mole and using standard enthalpies of formation:CaC(s) -> CaO(s) + C(g)A) -1207 kJ/molB) +1207 kJ/molC) - 851 kJ/molD) + 851 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 0.025 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) ΔH= ?A) -5.41 kJB) -90.0 kJC) -180 kJD) -364 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 for the reaction, as written.Ba(s) + 2 H2O(l) -> Ba(OH)2(aq) + H2(g) = ?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, absorbs 4.689 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) is its heat of fusion is and its heat of vaporization is 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) -3108 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 (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) ΔH = 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 J.A) -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.