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 rxn kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/°C.
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 rxn kJ/mol biphenyl. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.86 kJ/°C.
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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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Can you please answer question 5
![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 (C₂H) 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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa7634a6a-5ecc-40e2-9892-46ba7a4cefd4%2F6c2413e0-5c38-468a-92b9-2e1e0f1a805c%2F3thfpl3_processed.jpeg&w=3840&q=75)
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 (C₂H) 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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