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ThermochemistryCh5

 1) 

Given the equation

H2O (l) ® H2O (g)    DHrxn = 40.7 kJ at 100 °C

Calculate the mass of liquid water (in grams) at 100 °C that can converted to vapor by absorbing 2400 J of heat.
 

 2) 

A sample of aluminum metal absorbs 8.32 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is __________ g.
A)
72
B)
1.3
C)
7.5
D)
65
E)
7.3
 

 3) 

Given the equation

H2O (l) ® H2O (g)        DHrxn = 40.7 kJ at 100°C

Calculate the heat required to convert 3.00 grams of liquid water at 100 °C to vapor.
 

 4) 

The internal energy of a system __________.
A)
is the sum of the kinetic energy of all of its components
B)
is the sum of the rotational, vibrational, and translational energies of all of its components
C)
refers only to the energies of the nuclei of the atoms of the component molecules
D)
is the sum of the potential and kinetic energies of the components
E)
none of the above
 

 5) 

A 25.5-g piece of cheddar cheese contains 37% fat, 28% protein, and 4% carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value for this piece of cheese is __________ kJ.
 

 6) 

The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is __________ kcal.
 

 7) 

Given the data in the table below, Drxn for the reaction

4NH3 (g) + 5 O2 (g) ® 4NO (g) + 6 H2O (l)

is __________ kJ.

mc007-1.jpg
 

 8) 

Given the equation:

CH4 (g) + 2 O2 (g) ® CO2 (g) + H2O (l)     DH = -890 kJ

The heat liberated when 34.78 grams of methane (CH4) are burned in an excess amount of oxygen is __________ kJ.
 

 9) 

Given the following reactions
N2 (g) + O2 (g) ® 2NO (g)            DH = +180.7 kJ
2 N2O (g) ® O2 (g) + 2N2 (g)        DH = -163.2 kJ
the enthalpy of reaction for
2 N2O (g) ® 2NO (g) + N2 (g)

is __________ kJ.
 

 10) 

Which of the following statements is false?
A)
Internal energy is a state function.
B)
Enthalpy is an intensive property.
C)
The enthalpy change for a reaction is equal in magnitude, but opposite in sign, to the enthalpy change for the reverse reaction.
D)
The enthalpy change for a reaction depends on the state of the reactants and products.
E)
The enthalpy of a reaction is equal to the heat of the reaction.
 

 11) 

For which one of the following reactions is Drxn equal to the heat of formation of the product?
A)
N2 (g) + 3H2 (g) ® 2NH3 (g)
B)
(1/2) N2 (g) + O2 (g) ® NO2 (g)
C)
6C (s) + 6H (g) ® C6H6 (l)
D)
P (g) + 4H (g) + Br (g) ® PH4Br (l)
E)
12C (g) + 11H2 (g) + 11O (g) ® C6H22O11 (g)
 

 12) 

The value of DH° for the reaction below is +128.1 kJ:

CH3OH (l) ® CO (g) + 2 H2 (g)
How many kJ of heat are consumed when 15.5 g of CH3OH (l) decomposes as shown in the equation?
 

 13) 

The average fuel value of sugars is 17 kJ/g. A 2.0 L pitcher of sweetened Kool-Aid contains 400 g of sugar. What is the fuel value (in kJ) of a 500 mL serving of Kool-Aid? (Assume that the sugar is the only fuel source.)
 

 14) 

The value of DH° for the reaction below is -336 kJ. Calculate the heat (kJ) released to the surroundings when 23.0 g of HCl is formed.

CH4 (g) + 3 Cl2 (g) ® CHCl3 (l) + 3HCl (g)
 

 15) 

Under what condition(s) is the enthalpy change of a process equal to the amount of heat transferred into or out of the system?

(a) temperature is constant
(b) pressure is constant
(c) volume is constant
A)
a only
B)
b only
C)
c only
D)
a and b
E)
b and c
 

 16) 

Given the data in the table below, Drxn for the reaction

IF5 (g) + F2 (g) ® IF7 (g)

is __________ kJ.

mc016-1.jpg
 

 17) 

Given the following reactions

N2 (g) + 2 O2 (g) ® 2NO2 (g)       DH = 66.4 kJ

2NO (g) + O2 (g) ® 2NO2 (g)       DH = -114.2 kJ

the enthalpy of the reaction of the nitrogen to produce nitric oxide

N2 (g) + O2 (g) ® 2NO (g)

is __________ kJ.
 

 18) 

Calculate the kinetic energy in joules of an automobile weighing 4345 lb and traveling at 75 mph. (1 mile = 1.6093 km, 1 lb = 453.59 g)
 

 19) 

Given the data in the table below, Drxn for the reaction

Ca(OH)2 + 2 H3AsO4 ® Ca(H2AsO4)2 + 2 H2O

is __________ kJ.

mc019-1.jpg
 

 20) 

Calculate the kinetic energy in joules of an automobile weighing 2135 lb and traveling at 55 mph.  (1 mile = 1.6093 km, 1 lb = 453.59 g)
 

 21) 

Given the data in the table below, Drxn for the reaction

Ag2O (s) + H2S (g) ® Ag2S (s) + H2O (l)

is __________ kJ.

mc021-1.jpg
 

 22) 

A slice of apple pie contains 14.0 grams of fat, 2.00 grams of protein, and 52.0 grams of carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. If cycling typically burns 1000.0 kJ/hour, __________ minutes of cycling are required to completely burn off the slice of pie.
 

 23) 

The value of ÄH° for the reaction below is -1107 kJ:

2Ba (s) + O2 (g) ® 2BaO (s)

How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form
BaO (s)?
 

 24) 

When 0.800 grams of NaOH is dissolved in 100.0 grams of water, the temperature of the solution increases from 25.00 °C to 27.06 °C. The amount of heat absorbed by the water is __________ J. (The specific heat of water is 4.18 J/g- °C.)
 

 25) 

The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1 °C to 65.3 °C?
A)
48.1
B)
840
C)
1.89 ´ 103
D)
2.08 ´ 10-2
E)
54.4
 

 26) 

Given the data in the table below, Drxn for the reaction

PCl3 (g) + 3 HCl (g) ® 3 Cl2 (g) + PH3 (g)

is __________ kJ.

mc026-1.jpg
 

 27) 

The value of ÄH° for the reaction below is -6535 kJ. __________ kJ of heat are released in the combustion of 16.0 g of C6H6 (l)?

2 C6H6 (l) + 15 O2 (g) ® 12CO2 (g) + 6 H2O (l)
 

 28) 

A sample of calcium carbonate [CaCO3 (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams) of the sample?
A)
3.7
B)
5.0
C)
7.5
D)
410
E)
5.0 ´ 103
 

 29) 

The value of DH° for the following reaction is 177.8 kJ. The value of DHf° for CaO(s) is __________ kJ/mol.

CaCO3 (s) ® CaO (s) + CO2 (g)

mc029-1.jpg
 

 30) 

An 8.29 g sample of calcium carbonate [CaCO3 (s)] absorbs 50.3 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. What is the specific heat of calcium carbonate?
A)
.63
B)
.82
C)
1.1
D)
2.2
E)
4.2
 

 31) 

A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5 °C to 28.5 °C. If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams) of the sample?
A)
4.3
B)
11
C)
21
D)
1100
E)
1.1 ´ 103
 

 32) 

The kinetic energy of a 23.2-g object moving at a speed of 81.9 km/hr is __________ J.
 

 33) 

Given the following reactions

CaCO3 (s) ® CaO (s) + CO2 (g)            DH = 178.1 kJ
C (s, graphite) + O2 (g) ® CO2 (g)          DH = -393.5 kJ

the enthalpy of the reaction

CaCO3 (s) ® CaO (s) + C (s, graphite) + O2 (g)

is __________ kJ.
 

 34) 

A 5-ounce cup of raspberry yogurt contains 6.0 g of protein, 2.0 g of fat, and 20.2 g of carbohydrate. The fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. The fuel value of this cup of yogurt is __________ kJ.
A)
520
B)
630
C)
340
D)
720
E)
72
 

 35) 

The specific heat capacity of solid copper metal is 0.385 J/g-K. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0 °C to 77.5 °C?
A)
1.79 ´ 105
B)
26.6
C)
2.66 ´ 104
D)
5.58 ´ 10-6
E)
0.00558
 

 36) 

A 100-watt electric incandescent light bulb consumes __________ J of energy in 24 hours. [1 Watt (W) = 1 J/sec]
 

 37) 

The value of ÄE for a system that performs 111 kJ of work on its surroundings and gains 89 kJ of heat is __________ kJ.
A)
-111
B)
-200
C)
200
D)
-22
E)
22
 

 38) 

Given the data in the table below, ÄH°rxn for the reaction

3NO2 (g) + H2O (l) ® 2HNO3 (aq) + NO (g)

is __________ kJ.

mc038-1.jpg
 

 39) 

The temperature of a 15-g sample of lead metal increases from 22 °C to 37 °C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is __________ J/g-K.
 

 40) 

For which one of the following reactions is the value of Drxn equal to DHf° for the product?
A)
2Ca (s) + O2 (g) ® 2CaO (s)
B)
C2H2 (g) + H2 (g) ® C2H4 (g)
C)
2C (graphite) + O2 (g) ® 2CO (g)
D)
3Mg (s) + N2 (g) ® Mg3N2 (s)
E)
C (diamond) + O2 (g) ® CO2 (g)
 

 41) 

A 22.44 g sample of iron absorbs 180.8 J of heat, upon which the temperature of the sample increases from 21.1 °C to 39.0 °C. What is the specific heat of iron?
A)
0.140
B)
0.450
C)
0.820
D)
0.840
E)
0.900
 

 42) 

The value of DH° for the reaction below is -186 kJ. Calculate the heat (kJ) released from the reaction of 25 g of Cl2.

H2 (g) + Cl2 (g) ® 2HCl (g)
 

 43) 

Consider the following two reactions:

A ® 2B           Drxn = 456.7 kJ/mol
A ® C                  Drxn = -22.1kJ/mol

Determine the enthalpy change for the process:

2B ® C
A)
-478.8 kJ/mol
B)
-434.6 kJ/mol
C)
434.6 kJ/mol
D)
478.8 kJ/mol
E)
More information is needed to solve the problem.
 

 44) 

Given the following reactions:
2S (s) + 3O2 (g) ® 2SO3 (g)        DH = -790 kJ
S (s) + O2 (g) ® SO2 (g)              DH = -297 kJ

the enthalpy of the reaction in which sulfur dioxide is oxidized to sulfur trioxide

2SO2 (g) + O2 (g) ® 2SO3 (g)

is __________ kJ.
 

 45) 

Given the following reactions
(1) 2NO ® N2 + O2             DH = -180 kJ
(2) 2NO + O2 ® 2NO2        DH = -112 kJ

the enthalpy of the reaction of nitrogen with oxygen to produce nitrogen dioxide

N2 + 2O2 ® 2NO2

is __________ kJ.
 

 46) 

Given the data in the table below, Drxn for the reaction

3 Cl2 (g) + PH3 (g) ® PCl3 (g) + 3 HCl (g)

is __________ kJ.

mc046-1.jpg
 

 47) 

Which of the following is a statement of the first law of thermodynamics?
A)
Ek = mc047-1.jpg mv2
B)
A negative ÄH corresponds to an exothermic process.
C)
DE = Efinal – Einitial
D)
Energy lost by the system must be gained by the surroundings.
E)
1 cal = 4.184 J (exactly)
 

 48) 

The combustion of titanium with oxygen produces titanium dioxide:

Ti (s) + O2 (g) ® TiO2 (s)

When 2.060 g of titanium is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 91.60 °C. In a separate experiment, the heat capacity of the calorimeter is measured to be 9.84 kJ/K. The heat of reaction for the combustion of a mole of Ti in this calorimeter is __________ kJ/mol.
A)
14.3
B)
19.6
C)
-311
D)
-0.154
E)
-1.52 ´ 104
 

 49) 

The temperature of a 12.58 g sample of calcium carbonate [CaCO3 (s)] increases from 23.6 °C to 38.2 °C. If the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are absorbed?
A)
0.82
B)
5.0
C)
7.5
D)
410
E)
151
 

 50) 

The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.
 

 51) 

Given the data in the table below, DH°rxn for the reaction
SO3 (g) + H2O (l) ® H2SO4 (l)

is __________ kJ.

mc051-1.jpg
 

 52) 

The specific heat capacity of liquid mercury is 0.14 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of mercury from 15.0 °C to 36.5 °C?
A)
7.7 ´ 102
B)
15
C)
36
D)
0.0013
E)
1.7
 

 53) 

The value of DH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is __________ kJ.

2S (s) + 3O2 (g) ® 2SO3 (g)
 

 54) 

Given the following reactions

N2 (g) + O2 (g) ® 2NO (g)            DH = +180.7 kJ
2 N2O (g) ® O2 (g) + 2N2 (g)        DH = -113.1 kJ

the enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen
2 N2O (g) ® O2 (g) + 2N2 (g)

is __________ kJ.
 

 55) 

Given the data in the table below and Drxn for the reaction

SO2Cl2 (g) + 2 H2O (l)® H2SO4 (l) + 2HCl (g)       DH° = -62 kJ

DH°f of HCl (g) is __________ kJ/mol.

mc055-1.jpg
 

 56) 

The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0 °C to 75.0 °C?
A)
88.6
B)
429
C)
1221
D)
0.0113
E)
22.9
 

 57) 

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction:

      2H2O2 (l) ® 2H2O (l) + O2 (g)                    DH = -196 kJ

Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure?
A)
-23.1
B)
-11.5
C)
-0.0217
D)
1.44
E)
-2.31 ´ 104
 

 58) 

Given the following reactions
N2 (g) + O2 (g) ® 2NO (g)            DH = +180.7 kJ
2 N2O (g) ® O2 (g) + 2N2 (g)        DH = -113.1 kJ
the enthalpy of reaction for
      4NO (g) ® 2NO2 (g) + N2 (g)

is __________ kJ.
 

 59) 

A meal containing a burger, fries, and a milkshake contains 53.0 grams of fat, 38.0 grams of protein, and 152 grams of carbohydrate. The respective fuel values for protein, fat, and carbohydrate are 17, 38, and 17 kJ/g, respectively. If swimming typically burns 1100.0 kJ/hour, __________ minutes of swimming are required to completely burn off the meal.
 

 60) 

The value of DH° for the reaction below is -1107 kJ:

2Ba (s) + O2 (g) ® 2BaO (s)

How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen to form BaO (s)?
 

 61) 

The value of ÄH° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 6.00 g of CO (g) reacts completely.

2CO (g) + O2 (g) ® 2CO2 (g)
A)
1450
B)
103
C)
51.6
D)
482
E)
-482
 

 62) 

A 50.0-g sample of liquid water at 25.0 °C is mixed with 29.0 g of water at 45.0 °C. The final temperature of the water is __________ °C.
A)
102
B)
27.6
C)
35.0
D)
142
E)
32.3
 

 63) 

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water:

CH4 (g) + 2O2 (g) ® CO2 (g) + 2H2O (l)       DH = -890.0 kJ

Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.
A)
-94.6
B)
0.0306
C)
-0.0106
D)
32.7
E)
-9.46 ´ 104
 

 64) 

The value of DH° for the reaction below is -1107 kJ:

2Ba (s) + O2 (g) ® 2BaO (s)

How many kJ of heat are released when 5.75 g of BaO (s) is produced?
 

 65) 

The value of DH° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 38.5 g of O2 (g) reacts with excess CO.

2CO (g) + O2 (g) ® 2CO2 (g)
 

 66) 

Given the data in the table below, Drxn for the reaction

2SO2 (g) + O2 (g) ® 2SO3 (g)

is __________ kJ.

mc066-1.jpg
 

 67) 

The ÄH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 10.1-g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0 °C to __________°C. Assume that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K.
A)
35.2
B)
24.0
C)
33.7
D)
33.3
E)
40.2
 

 68) 

Given the data in the table below, DH°rxn for the reaction

      C2H5OH (l) + O2 (g) ? CH3CO2H (l) + H2O (l)

is __________ kJ.

mc068-1.jpg
 

 69) 

Given the following reactions

H2O (l) ® H2O (g)                            DH = 44.01 kJ
2 H2 (g) + O2 (g) ® 2 H2O (g)          DH = -483.64 kJ

the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen

2 H2O (l) ® 2 H2 (g) + O2 (g)

is __________ kJ.
 

 70) 

At what velocity (m/s) must a 20.0 g object be moving in order to possess a kinetic energy of 1.00 J?
A)
1.00
B)
100 ´ 102
C)
10.0
D)
1.00 ´ 103
E)
50.0
 

 71) 

The British thermal unit (Btu) is commonly used in engineering applications. A Btu is defined as the amount of heat required to raise the temperature of 1 lb of water by 1 °F. There are __________ joules in one Btu. 1 lb = 453.59 g; °C = (5/9)(°F - 32°); specific heat of H2O (l) = 4.184 J/g-K.
A)
3415
B)
60.29
C)
1054
D)
5.120 ´ 10-3
E)
Additional information is needed to complete the calculation.
 

 72) 

A 5.00-g sample of liquid water at 25.0 °C is heated by the addition of 84.0 J of energy. The final temperature of the water is __________ °C. The specific heat capacity of liquid water is 4.18 J/g-K.
A)
95.2
B)
25.2
C)
-21.0
D)
29.0
E)
4.02
 

 73) 

Given the data in the table below, DH° for the reaction
2CO (g) + O2 (g) ® 2CO2 (g)

is __________ kJ.

mc073-1.jpg
 

 74) 

Calculate the kinetic energy in J of an electron moving at 6.00 ´ 106 m/s. The mass of an electron is 9.11 ´ 10-28 g.
 

 75) 

The value of DH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 20.0 g of Na2O2 with water is __________ kJ.

2 Na2O2 (s) + 2 H2O (l) ® 4NaOH (s) + O2 (g)
A)
16.2
B)
32.3
C)
67.5
D)
64.6
E)
-126
 

 76) 

The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22 °C to 37 °C?
 

 77) 

Which one of the following statements is true?
A)
Enthalpy is an intensive property.
B)
The enthalpy change for a reaction is independent of the state of the reactants and products.
C)
Enthalpy is a state function.
D)
H is the value of q measured under conditions of constant volume.
E)
The enthalpy change of a reaction is the reciprocal of the ÄH of the reverse reaction.
 

 78) 

The value of DH° for the reaction below is +128.1 kJ:

CH3OH (l) ® CO (g) + 2 H2 (g)

How many kJ of heat are consumed when 5.10 g of CO (g) is formed as shown in the equation?
 

 79) 

The temperature of a 35.2 g sample of iron increases from 23.7 °C to 29.5 °C. If the specific heat of iron is 0.450 J/g-K, how many joules of heat are absorbed?
A)
4.3
B)
92
C)
0.450
D)
1100
E)
1.1 ´ 103
 

 80) 

For which one of the following equations is Drxn equal to DHf° for the product?
A)
Xe (g) + 2 F2 (g) ® XeF4 (g)
B)
CH4 (g) + 2 Cl2 (g) ® CH2 Cl2 (l) + 2HCl (g)
C)
N2 (g) + O3 (g) ® N2O3 (g)
D)
2CO (g) + O2 (g) ® 2CO2 (g)
E)
C (diamond) + O2 (g) ® CO2 (g)
 

 81) 

Given the following reactions
Fe2O3 (s) + 3CO (s) ? 2Fe (s) + 3CO2 (g)       DH = -28.0 kJ

3Fe (s) + 4CO2 (s) ? 4CO (g) + Fe3O4 (s)       DH = +12.5 kJ

the enthalpy of the reaction of Fe2O3 with CO

3 Fe2O3 (s) + CO (g) ? CO2 (g) + 2 Fe3O4 (s)

is __________ kJ.
 

 82) 

A 6.50-g sample of copper metal at 25.0 °C is heated by the addition of 84.0 J of energy. The final temperature of the copper is __________°C. The specific heat capacity of copper is 0.38 J/g-K.
A)
29.9
B)
25.0
C)
9.0
D)
59.0
E)
34.0
 

 83) 

Given the data in the table below, Drxn for the reaction

2 AglS (s) + O2 (g) ® 2 Ag2O (s) + 2S (s)

is __________ kJ.

mc083-1.jpg
 

 84) 

The value of DH° for the reaction below is +128.1 kJ:

CH3OH (l) ® CO (g) + 2 H2 (g)

How many kJ of heat are consumed when 5.10 g of H2 (g) is formed as shown in the equation?
 

 85) 

The value of DH° for the reaction below is +128.1 kJ:

CH3OH (l) ® CO (g) + 2 H2 (g)

How many kJ of heat are consumed when 5.75 g of CO (g) is formed as shown in the equation?
 

 86) 

What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 mL of solution having a density of 1.25 g/mL by 7.80 °C? (The specific heat of the solution is 3.74 joules/gram-K.)
A)
-7.43
B)
-12.51
C)
8.20
D)
-9.12
E)
6.51
 

 87) 

The molar heat capacity of a compound with the formula C2H6SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.
 

 88) 

Of the following, DHf° is not zero for __________.
A)
Sc (g)
B)
Si (s)
C)
P4 (s, white)
D)
Br2 (l)
E)
Ca (s)
 

 89) 

The specific heat of bromine liquid is 0.226 J/g K. The molar heat capacity (in J/mol-K) of bromine liquid is __________.
 

 90) 

ÄH for the reaction

IF5 (g) ® IF3 (g) + F2 (g)

is __________ kJ, give the data below.

IF (g) + F2 (g) ® IF3 (g)              DH = -390 kJ

IF (g) + 2 F2 (g) ® IF5 (g)          DH = -745 kJ
 



 
         Start Over

Nuclear Videos

Intro Video Near the end she discusses balancing equations.


Half Life Video