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Q:
Find H for C3H8 (g) + 6 H2O (g) -> 3 CO2 (g) + 10 H2given C3H8 (g) + 3 H2O (g) -> 3 CO (g) + 7 H2 (g) H = 499 kJCO (g) + H2O (g) -> CO2 (g) + H2 (g) H = -41 kJA) 376 kJB) 458 kJC) 540 kJD) 622 kJ
Q:
Find H for BaCO3 (s) -> BaO (s)+ CO2 (g)given 2 Ba (s) + O2 (g) -> 2 BaO (s) H = -1107.0 kJBa (s) + CO2 (g) + 1/2 O2 (g) -> BaCO3 (g) H = -822.5 kJA) -1929.5 kJB) -1376.0 kJC) -284.5 kJD) 269.0 kJ
Q:
Coal gasification can be represented by the equation:2 C(s) + 2 H2O(g) -> CH4(g) + CO2(g) H = ?Use the following information to find H for the reaction above.CO(g) + H2(g) -> C(s) + H2O(g) H = -131 kJCO(g) + H2O(g) -> CO2(g) + H2(g) H = -41 kJCO(g) + 3 H2(g) -> CH4(g) + H2O(g) H = -206 kJA) 15 kJB) 116 kJC) -116 kJD) -372 kJ
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 4.18 J/(g C), 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 is4.18 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) -362 kJ
Q:
Water has an unusually high
A) 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/(g C).A) aluminum (0.902)B) copper (0.385)C) Gold (0.129)D) iron (0.450)
Q:
Which is expected to have the lowest specific heat capacity at 25C?
A) air
B) copper
C) polyethylene
D) water
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
0.857 J/(gC), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol.
A) 1.11 kJ
B) 1.64 kJ
C) 5.96 kJ
D) 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) -3120 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:
At a constant pressure of 1.50 atm what is the enthalpy change H for a reaction where the internal energy change E is 58.0 kJ and the volume increase is 12.6 L? (1 Latm = 101.325 J.)A) 39.1 kJB) 56.1 kJC) 59.9 kJD) 76.9 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 H 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:
At constant pressure for the reaction shown below, 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 decrease 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) temperature
D) work
Q:
A slice of cheese pizza has a caloric content of 150 Cal. If this energy could be used to power a 2500 Watt microwave oven, how many minutes could the microwave oven be operated?
A) 1.0 min
B) 4.2 min
C) 11 min
D) 15 min
Q:
For a system at constant pressure, 12,400 calories of heat are released. This quantity of heat is equivalent to
A) 1.92 10-5 J.
B) 2.96 103 J.
C) 1.24 104 J.
D) 5.19 104 J.
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:
At 253 K the sign of G for the physical change shown below is ________.H2O(s) -> H2O(l)
Q:
The sign of G for a reaction is if the reaction is spontaneous, ________ if the reaction is at equilibrium, and ________ if the reaction is nonspontaneous.
Q:
A spontaneous reaction has a ________ value of G and is favored by a ________ value of H and a ________ value of S.
Q:
The sign of S for reaction below is expected to be ________.2 H2(g) + O2(g) -> 2 H2O(g)
Q:
For the reaction: A + 2 B -> 3 C, H = -203 kJ. For the reaction 6 C -> 2 A + 4 B, H = ________ kJ.
Q:
Heat transfer measured in a coffee-cup calorimeter at constant pressure is a measure of ________, but heat transfer measured in a bomb calorimeter at constant volume is a measure of ________.
Q:
A reaction is performed in a water bath initially at 21C which decreases to 18C by the end of the reaction. For this reaction the sign of heat transfer is ________, and the reaction is classified as ________.
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:
A reaction that absorbs 49.6 kJ from the surroundings in a vessel that undergoes a volume decrease of 1.25 L at a constant 4.00 atm pressure has an energy change, E = ________ kJ.
Q:
A reaction is performed in a 1-L balloon at 25C and 1 atm pressure. At the end of the reaction the balloon has expanded to 1.5 L and the surface of the balloon has a temperature of 35C and is at 1 atm pressure. Determine whether the signs of the heat transferred, the work, and the energy change, respectively, are positive or negative.
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:
When the reaction below is performed in a water bath, will the temperature of the water bath increase or decrease?432 kJ + A + 2 B -> 3 C
Q:
In the reaction below, is energy released or absorbed by the system? What is the sign of the energy change, E?432 kJ + A + 2B -> 3C
Q:
A property whose value depends only on the present condition of the system and not how the system arrived at that condition is called a ________ function.
Q:
The sum of the potential and kinetic energies for every molecule or ion in a system is the ________ energy of the system and is given the symbol ________.
Q:
Is chemical energy a form of kinetic or potential molecular energy?
Q:
Is thermal energy a form of kinetic or potential molecular energy?
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:
The law of conservation of energy is also known as the ________ law of thermodynamics.
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:
For the reaction, CH4(g) -> C(g) + 4 H(g), one would expectA) H to be negative and S to be negative.B) H to be negative and S to be positive.C) H to be positive and S to be negative.D) H to be positive and S to be positive.