5. When 0.514 g of biphenyl (CH) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8°C to 29.4°C. Find the AE for the combustion of biphenyl in kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/°C. rxn
5. When 0.514 g of biphenyl (CH) undergoes combustion in a bomb calorimeter, the temperature rises from 25.8°C to 29.4°C. Find the AE for the combustion of biphenyl in kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/°C. rxn
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.31QP: Chemical reactions are run in each of the beakers depicted below (labeled A, B, and C). The...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Can you please answer question 5 without using the specific heat of byphenyl
Transcribed Image Text:1. When 1 mol of a fuel is burned at constant pressure, it
produces 3452 kJ of heat and does 11 kJ of work. What are
the values of ΔΕ and ΔΗ?
2. A gas is compressed from an initial volume of 5.55 L to a
final volume of 1.22L at an external pressure of 1.00 atm.
During the compression, 124 J of heat are released. What
is the AE (in J)?
3. A piece of copper metal whose mass is 3.45 g is heated to
95.0°C and then dropped onto a calorimeter made of ice at
0.0°C. As the metal cools to 0.0°C, 0.372 g of the ice melts
(AH (water)=6.01 kJ/mol). From this experiment, find the
molar heat capacity (in J/°C*mol) of the copper.
4. In order to measure the enthalpy change for the reaction
that occurs in instant cold packs used by athletes, 1.25 g of
NH NO, is dissolved in enough water to make 25.0 mL of
solution. Th initial temperature is 25.8°C and the fina
temperature is 21.9°C. Calculate the AH for the dissolution
reaction below in kJ/mol. Assume that the specific heat
capacity of the solution is 4.18 J/g*°C and that its density
1.00 g/mL and that the calorimeter itself absorbs a
negligible amount of heat.
NH4NO3(s) à NH4+ (aq) + NO3(aq)
5. When 0.514 g of biphenyl (CH) undergoes combustion in
a bomb calorimeter, the temperature rises from 25.8°C to
29.4°C. Find the AE for the combustion of biphenyl in
kJ/mol biphenyl. The heat capacity of the bomb
calorimeter, determined in a separate experiment, is 5.86
kJ/°C.
6. Use Hess's Law and the following data:
Sro(s) à Sr (s) + 1/2O₂(g)
SrO(s) + CO₂(g) à SrCO3(s)
2 CO₂(g) à 2 C(graphite) + 2 O₂(g)
AH°= +592 kJ
AH°= -234kJ
AH°=+788 kJ
to determine the standard heat of formation AH (in kJ) for
strontium carbonate (SrCO3). Strontium carbonate emits a
brilliant red colour in flames and due to its low cost, is used
in fireworks.
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