Trinitroglycerin, C3H5N3O9 (usually referred to simply as nitroglycerin), has been widely used as an explosive. Alfred Nobel usedit to make dynamite in 1866. Rather surprisingly, it also is used as a medication, to relieve angina (chest pains resulting frompartially blocked arteries to the heart) by dilating the blood vessels. At 1 atm pressure and 25 °C, the enthalpy of decompositionof trinitroglycerin to form nitrogen gas, carbon dioxide gas, liquid water, and oxygen gas is -1541.4 kJ/mol.(a) Write a balanced chemical equation for the decomposition of trinitroglycerin.(b) Calculate the standard heat of formation of trinitroglycerin.(c) A standard dose of trinitroglycerin for relief of angina is 0.60 mg. If the sample is eventually oxidized in the body (not explosively,though!) to nitrogen gas, carbon dioxide gas, and liquid water, what number of calories is released?(d) One common form of trinitroglycerin melts at about 3 °C. From this information and the formula for the substance, would youexpect it to be a molecular or ionic compound? Explain.(e) Describe the various conversions of forms of energy when trinitroglycerin is used as an explosive to break rockfaces in highwayconstruction.
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.
Trinitroglycerin, C3H5N3O9 (usually referred to simply as nitroglycerin), has been widely used as an explosive. Alfred Nobel used
it to make dynamite in 1866. Rather surprisingly, it also is used as a medication, to relieve angina (chest pains resulting from
partially blocked arteries to the heart) by dilating the blood vessels. At 1 atm pressure and 25 °C, the enthalpy of decomposition
of trinitroglycerin to form nitrogen gas, carbon dioxide gas, liquid water, and oxygen gas is -1541.4 kJ/mol.
(a) Write a balanced chemical equation for the decomposition of trinitroglycerin.
(b) Calculate the standard heat of formation of trinitroglycerin.
(c) A standard dose of trinitroglycerin for relief of angina is 0.60 mg. If the sample is eventually oxidized in the body (not explosively,
though!) to nitrogen gas, carbon dioxide gas, and liquid water, what number of calories is released?
(d) One common form of trinitroglycerin melts at about 3 °C. From this information and the formula for the substance, would you
expect it to be a molecular or ionic compound? Explain.
(e) Describe the various conversions of forms of energy when trinitroglycerin is used as an explosive to break rockfaces in highway
construction.
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