Question

Can I have help with these questions based off the information provided?

Information:

The explosive picric acid is also known by the IUPAC name 2,4,6-Trinitrophenol. Picric acid is known as a primary explosive and the balanced equation for the explosion is

4 C₆H₃N₃ O₇ (aq) + 13 O₂ (g) --> 6 H₂O (g) + 6 N₂ (g) + 24 CO₂ (g)

volume of gas produced by 1 g is 0.89 L

Type bond broken	# bond type	Enthalpy (KJ/mol	Total energy (KJ/mol)		Type bond made	# bond type	Enthalpy (KJ/mol	Total energy (KJ/mol)
O-C	4	350	1400		O-H	12	464	5568
O-H	4	464	1856		N (triple bond) N	6	946	5676
C-C	24	345	8280		O=C	48	799	38352
C-H	8	415	3320
C-N	12	290	3480
N=O	12	600	7200
N-O	12	200	2400
O=O	13	498	6474

Questions:

1. Your textbook states “A standard enthalpy of formation ΔHf is an enthalpy change for a reaction in which exactly 1 mole of a pure substance is formed from free elements in their most stable states under standard state conditions. These values are especially useful for computing or predicting enthalpy changes for chemical reactions that are impractical or dangerous to carry out, or for processes for which it is difficult to make measurements. I think that sounds like explosive reactions!
   1. Using the enthalpy of formations from appendix G of your text and the enthalpy of reaction determined in 2) above, calculate a theoretical enthalpy of formation for your explosive compound. Remember,

ΔHrxn=∑n×ΔHf0(products)−∑n×ΔHf0(reactants)

Explain all you work to help everyone (and yourself), understand your calculations.

1. 2. Comment on the sign and magnitude of the enthalpy of formation for your explosive. Is it large positive or large negative? What does the positive or negative mean anyway?
2. We can all agree an explosion does work! A type of work called expansion work (or pressure-volume work) occurs when a system that produces gases pushes back the surroundings against an outside pressure. Remember the volume of gas produced from the 1 gram of your explosive? Given the volume of gas produced, determine the work done (in kJ) upon the expansion of the gases from the explosion of 1 g of explosive. Assume the atmospheric pressure is 1 atmosphere. Remember, w = -PDV and the conversion factor for Joules and change in volume against a pressure is 1 L atm = 101.3 Joules.
3. Back to heat produced from an explosion! Determine the heat energy (kJ) produced from a 1 kg amount of your explosive by using the enthalpy of reaction you determined above in number 2.
4. Your explosive reaction from 2. above should have resulted in a negative enthalpy change, which is indicative of an exothermic reaction. Remembering the definition of “exothermic”, write a sentence or two on how this “exothemicity” may affect the value for the volume of gas you used to calculate expansion work in #2.