Department of Biochemistry
Semester IV ASSIGNMENT- 16UBCCC13 Membrane Biology and Bioenergetics
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One mole of gas absorbs 44 J of heat. If th work done on the surrounding by the gas is
25J, then calculate delta U for the gas .
You do 450 kJ of work on bicycle and lose 55 kJ of energy as heat. What is the change
in your internal energy?
To make iron, a steel mill takes Fe2O3 (rust or iron ore) and reacts it with coke (a
complex, impure form of carbon) to make iron and CO2. Based on the data below, this
is a non-spontaneous reaction at room temperature, but it becomes spontaneous at
higher temperatures. Assuming that H° and S° do not change much with
temperature, calculate the temperature above which the reaction becomes spontaneous
(i.e., G° rxn = 0).
H° rxn = +465 kJ/mol
S° rxn = +552 J/molK (or 0.552 kJ/molK)
G° rxn = +301 kJ/mol (at 298 K)
Determine the standard entropy change and Calculate ∆G° for the decomposition of
one mole of solid calcium carbonate, forming solid calcium oxide and carbon dioxide
gas. CaCO3(s) → CaO(s) + CO2(g)
∆H° = (1 mol)[∆H° for CaO(s)] + (1 mol)[∆H° for CO2(g)] – (1 mol)[∆H° for
CaCO3(s)] = (1 mol)) + (1 mol)) – (1 mol)) = 178.2 kJ
∆S0
∆H0
CaO(s)
39.8 J/mol K
–635.3 kJ/mol
CO2(g)
213.7 J/mol K
–393.5 kJ/mol
CaCO3)(s
(92.9 J/mol K)
–1207.0 kJ/mol
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