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ChemistryQ&A LibraryLiquid trinitroglycerin (C3H5N3O9) has been widely used as an explosive and as a medication to relieve angina. The enthalpy of decomposition (ΔHdec) for C3H5N3O9 to form N2(g), CO2(g), H2O(l), and O2(g) is -1541.4 kJ/mol.1. Write the thermochemical equation for the decomposition of 1 mole of trinitroglycerin. 2. Calculate the standard heat of formation (ΔHf) for C3H5N3O9.3. A standard does of C3H5N3O9 for relief of angina is 0.60 mg. If a sample is eventually oxidized completely, how many calories are released?Question

Asked Dec 13, 2019

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Liquid trinitroglycerin (C3H5N3O9) has been widely used as an explosive and as a medication to relieve angina. The enthalpy of decomposition (ΔHdec) for C3H5N3O9 to form N2(g), CO2(g), H2O(l), and O2(g) is -1541.4 kJ/mol.

1. Write the thermochemical equation for the decomposition of 1 mole of trinitroglycerin.

2. Calculate the standard heat of formation (ΔHf) for C3H5N3O9.

3. A standard does of C3H5N3O9 for relief of angina is 0.60 mg. If a sample is eventually oxidized completely, how many calories are released?

Step 1

The thermochemical equation for decomposition of 1 mol of trinitroglycerin is shown below:

Step 2

The standard heat of formation is calculated from the balanced equation of decomposition of trinitroglycerin. The balanced equation is shown below:

4C3H5N3O9(*l*)→6N2(*l*) + 12CO2(*g*) + 10H2O(*l*) + O2(g)

The enthalpy change for the above reaction is 4(-1541.4 kJ). The value of heat o...

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