Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ-K-'), together with 2.50 kg water. 2.2 After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-')
Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ-K-'), together with 2.50 kg water. 2.2 After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in internal energy of methanol (in kJ-mol-')
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.35QP: A 250-g sample of water at 20.0C is placed in a freezer that is held at a constant temperature of...
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Please answer 2.2 Only.
![2.1
Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in
methanol can be utilized in a multitude of reactions. Consider the following reaction for the
decomposition of methanol:
2CH;OH(f) → 2CH4(g) + 02(g)
Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known
thermochemical data:
H20(?) → /202(g) + H2(g)
CH4(g) + H20(g)→ 3H2(g) + CO(g)
2H2 (g) + CO(g) → CH3OH(?)
H20(g) → H20(t)
ДН, — 285.8 k] -тol-1
ДН, — 206.1 k] :тol-1
ΔΗ
ДН, 3D —128.3 k) : тol-1
ΔΗ
Дн, 3D — 44.00 k] -тol-1
[5]
2.2
Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol
was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ.K-'), together with 2.50 kg water.
After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in
internal energy of methanol (in kJ-mol-')
[5]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe919d4e8-7ddb-410a-93c7-896844b189cf%2Fdd57a9ae-7dbe-4525-9f19-d1672b3690be%2Fvlnd0eq_processed.png&w=3840&q=75)
Transcribed Image Text:2.1
Methanol is an attractive fuel source in a sustainable, green economy. The chemical energy inherent in
methanol can be utilized in a multitude of reactions. Consider the following reaction for the
decomposition of methanol:
2CH;OH(f) → 2CH4(g) + 02(g)
Use Hess' Law to calculate the enthalpy change (in kJ-mol-1) of this reaction, given the following known
thermochemical data:
H20(?) → /202(g) + H2(g)
CH4(g) + H20(g)→ 3H2(g) + CO(g)
2H2 (g) + CO(g) → CH3OH(?)
H20(g) → H20(t)
ДН, — 285.8 k] -тol-1
ДН, — 206.1 k] :тol-1
ΔΗ
ДН, 3D —128.3 k) : тol-1
ΔΗ
Дн, 3D — 44.00 k] -тol-1
[5]
2.2
Methanol can also be combusted in the presence of oxygen in order to release its energy. 16.0 g of methanol
was placed in a bomb calorimeter (with a known heat capacity of 1.37 kJ.K-'), together with 2.50 kg water.
After methanol was combusted, the temperature of the water increased by 30 °C. Calculate the change in
internal energy of methanol (in kJ-mol-')
[5]
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