Chem question! With reference to the "Chemistry at Work" box on explosives, use bond enthalpies to estimate the enthalpy change for the explosion of 1.00 g of nitroglycerin.

I found that the answer is 7.85 KJ, but how?

Question

Chemistry

Andrews

18 October, 23:03

Chem question! With reference to the "Chemistry at Work" box on explosives, use bond enthalpies to estimate the enthalpy change for the explosion of 1.00 g of nitroglycerin.

I found that the answer is 7.85 KJ, but how?

+2

Answers (1)

Know the Answer?

Macy Yoder · Answer 1

The mass of nitroglycerin is 1 g,

Molar mass of nitroglycerin is 227 g/mol

The number of moles = moles/molar mass

= 1 g / 227 g/mol

= 0.004405 mol

The equation for the bond enthalpy of the reaction is shown below, thus, the total enthalpy change in the reaction is as follows:

ΔHreaction = Number of moles (∑ΔHbond break - ∑ΔH bond forms)

= 0.004405 mol * - 3564.5 kJ/mol

= - 7.85 kJ

Chem question! With reference to the "Chemistry at Work" box on explosives, use bond enthalpies to estimate the enthalpy change for the explosion of 1.00 g of nitroglycerin.I found that the answer is 7.85 KJ, but how?

Chem question! With reference to the "Chemistry at Work" box on explosives, use bond enthalpies to estimate the enthalpy change for the explosion of 1.00 g of nitroglycerin.

I found that the answer is 7.85 KJ, but how?