Trinitroglycerin, C3H5N3O9C3H5N3O9 (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 0.65 mg. If the sample is eventually oxidized in the body to nitrogen gas, carbon dioxide gas, and liquid water, how many joules of energy is released? (d) If 2.5 calories is released upon the oxidation of trinitroglycerin in the body, how many μg of trinitroglycerin was taken?

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