CH 104: HEATS OF REACTION
• A calorimeter is used to measure the
amount of heat absorbed or released
during a chemical reaction.
• In today’s experiment you will measure the
heat of a reaction in a calorimeter that is
made out of 2 Styrofoam coffee cups.
• The inner cup holds an aqueous reaction
mixture. The outer cup gives additional
thermal insulation from the surrounding
environment. The thermometer is used to
measure the initial and final temperatures
of the reaction mixture.
CALORIMETRY
• The first law of thermodynamics says that energy, in all its forms, is
conserved in all processes. Or the heat lost (qlost) by a system equals
the heat gained (qgained) by the surroundings.
qlost + qgained = 0
• The fundamental equation of calorimetry says the heat lost by a
reaction (qlost = qreaction) is gained by the surrounding water and
calorimeter (qgained = qwater + qcalorimeter).
qreaction + qwater + qcalorimeter = 0
• q is negative if
heat is lost.
• q is positive if
heat is gained.
• q is measured
in joules (J).
CALORIMETRY
• Again, the fundamental equation of calorimetry is
qreaction + qwater + qcalorimeter = 0
• 4.184 joules (J) are needed to heat 1 gram (g) of water 1 degree Kelvin
(K). This is the specific heat of water. Therefore, the heat gained by
the water is
• And the heat gained by the calorimeter is
qcalorimeter = (heat capacity of the calorimeter) x (Tfinal – Tinitial)
Where
• The mass of water is in grams.
• The heat capacity of each calorimeter is unique. Therefore, in today’s
experiment you will measure the heat capacity of your calorimeter.
• Tfinal is the final temperature of the water in either Kelvin or Celsius.
• Tinitial is the initial temperature of the water in either Kelvin or Celsius.
• Why can these temperatures be measured in either Kelvin or Celsius?
• A Kelvin degree is the same size as a Celsius degree. Therefore, the
change in temperature is the same if it is measured in either Kelvin or
Celsius.
CALORIMETRY
• Again, the fundamental equation of calorimetry is
qreaction + qwater + qcalorimeter = 0
• Or
qreaction = –(qwater + qcalorimeter)
• Then substituting
MEASURING THE HEAT CAPACITY OF YOUR CALORIMETER
• In today’s experiment you will measure the heat capacity of your
calorimeter.
• A student puts 75.0 g water in a calorimeter. The temperature of this
water and the calorimeter is 21.4° C. Then he adds 74.5 g of water at
58.0° C. The final temperature of this mixture is 37.6° C. The specific
heat of water is 4.184 Jg-1K-1.
• How much heat was lost by the hot water?
qwater = 4.184 Jg-1K-1 x 74.5 g x (37.6° C – 58.0° C) = –6.36x103 J
• How much heat was gained by the cold water?
qwater = 4.184 Jg-1K-1 x 75.0 g x (37.6° C – 21.4° C) = 5.08x103 J
MEASURING THE HEAT CAPACITY OF YOUR CALORIMETER
• How much heat was gained by the calorimeter?
qlost + qgained = 0
qlost by water + qgained by water + qgained by calorimeter = 0
qgained by calorimeter = –(qlost by water + qgained by water)
qgained by calorimeter = –(–6.36x103 J + 5.08x103 J) = 1.28x103 J
• What is the heat capacity of the calorimeter?
Heat Capacity of the Calorimeter =
qgained by calorimeter / (Tfinal – Tinitial) =
1.28x103 J / (37.6° C – 21.4° C) = 78.7 JK-1
Heat capacity MUST be positive. If the calculated heat
capacity of your calorimeter is negative, it is wrong.
HEAT OF REACTION
• For a solution, the fundamental equation of calorimetry is
qreaction = –(qsolution + qcalorimeter)
• Or
• qreaction is called the heat of reaction. If qreaction is measured
at constant pressure, like in our calorimeters which are at
atmospheric pressure, then qreaction is also called the
change in enthalpy (ΔH).
• The change in enthalpy per mole reaction is sometimes
written as
.
MEASURING THE HEAT OF A REACTION
• In today’s experiment you will measure the change in enthalpy (
the following reaction.
) for
Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)
• A student puts 100. mL of 2.0 M HCl(aq) (an excess) in a calorimeter.
The temperature of this aqueous solution and the calorimeter is 21.4°
C. Then he adds 0.252 g of Mg(s). The final mass of this solution is 100.
g. The final temperature of this solution is 31.1° C. The specific heat of
this solution is 3.62 Jg-1K-1. Assume the heat capacity of the
calorimeter is 78.7 JK-1.
• How much heat was gained by the solution?
qsolution = 3.62 Jg-1K-1 x 100. g x (31.1° C – 21.4° C) = 3.5x103 J
MEASURING THE HEAT OF A REACTION
• A student puts 100. mL of 2.0 M HCl(aq) (an excess) in a calorimeter.
The temperature of this aqueous solution and the calorimeter is 21.4°
C. Then he adds 0.252 g of Mg(s). The final mass of this solution is 100.
g. The final temperature of this solution is 31.1° C. The specific heat of
this solution is 3.62 Jg-1K-1. Assume the heat capacity of the
calorimeter is 78.7 JK-1.
Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)
• How much heat was gained by the calorimeter?
qcalorimeter = (heat capacity of the calorimeter) x (Tfinal – Tinitial)
qcalorimeter = 78.7 JK-1 x (31.1° C – 21.4° C) = 7.6x102 J
MEASURING THE HEAT OF A REACTION
• A student puts 100. mL of 2.0 M HCl(aq) (an excess) in a calorimeter.
The temperature of this aqueous solution and the calorimeter is 21.4°
C. Then he adds 0.252 g of Mg(s). The final mass of this solution is 100.
g. The final temperature of this solution is 31.1° C. The specific heat of
this solution is 3.62 Jg-1K-1. Assume the heat capacity of the
calorimeter is 78.7 JK-1.
Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)
• How much heat was evolved by the reaction?
qreaction = –(qsolution + qcalorimeter)
qreaction = –(3.5x103 J + 7.6x102 J) = –4.3x103 J
MEASURING THE HEAT OF A REACTION
• A student puts 100. mL of 2.0 M HCl(aq) (an excess) in a calorimeter.
The temperature of this aqueous solution and the calorimeter is 21.4°
C. Then he adds 0.252 g of Mg(s). The final mass of this solution is 100.
g. The final temperature of this solution is 31.1° C. The specific heat of
this solution is 3.62 Jg-1K-1. Assume the heat capacity of the
calorimeter is 78.7 JK-1.
Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)
• How many moles of Mg(s) reacted? The atomic weight of Mg is 24.305
g/mole.
0.252 g of Mg /24.305 g of Mg mole-1 = 0.0104 moles of Mg
MEASURING THE HEAT OF A REACTION
• A student puts 100. mL of 2.0 M HCl(aq) (an excess) in a calorimeter.
The temperature of this aqueous solution and the calorimeter is 21.4°
C. Then he adds 0.252 g of Mg(s). The final mass of this solution is 100.
g. The final temperature of this solution is 31.1° C. The specific heat of
this solution is 3.62 Jg-1K-1. Assume the heat capacity of the
calorimeter is 78.7 JK-1.
Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq)
• What is the heat of reaction in kJ/mole?
SAFETY
• Give at least 1 safety concern for the following procedures that will be
used in today’s experiment.
• Heating with a flame.
• Injury from a burn or causing a fire. Be careful. Do not wear loose
clothing or long hair. Glass can shatter when heating; wear your
goggles at all times.
• Using 2.0 M HCl, and Mg(s).
• These are irritants. Wear your goggles at all times. Immediately clean
all spills. If you do get either of these in your eye, immediately flush
with water.
• Generating H2(g).
• Hydrogen gas is flammable. Do NOT generate H2(g) until all the Bunsen
burners in the laboratory are extinguished. Wear your goggles at all
times.
• Your laboratory manual has an extensive list of safety procedures.
Read and understand this section.
• Ask your instructor if you ever have any questions about safety.
SOURCES
• Barnes, D.S., J.A. Chandler. 1982. Chemistry 111-112
Workbook and Laboratory Manual. Amherst, MA: University
of Massachusetts.
• McMurry, J., R.C. Fay. 2004. Chemistry, 4th ed. Upper
Saddle River, NJ: Prentice Hall.
• Petrucci, R.H. 1985. General Chemistry Principles and
Modern Applications, 4th ed. New York, NY: Macmillan
Publishing Company.