1. An explosive with a formula weight of 341.5 g/mole and a heat of formation of

Question

1. An explosive with a formula weight of 341.5 g/mole and a heat of formation of -421.6 kJ/mole detonates and produces elemental nitrogen, hydrogen, CO(g), CO2(g), and H2O(g). If 1 moles of explosive generates 3 moles of CO, 2 moles of CO2, and 7 moles of water, what is the heat of reaction for the detonation? Report in kJ/mole of the explosive, no decimals, and with the correct sign. Use the heats of formation from the text and assume gases are formed.

2. An explosive with a formula weight of 249 g/mole and a heat of formation of -424 kJ/mole detonates and produces elemental nitrogen, hydrogen, CO(g), CO2(g), and H2O(g). If 1 moles of explosive generates 4 moles of CO, 5 moles of CO2, and 3 moles of water, what is the heat released (Q) per gram detonated? Report in kJ/g with one decimal place. Assume Q is postive.

3.

A cartridge is loaded with 88.5 grains of propellant that releases 1,091.2 kcal/kg of energy when burned. If the conversion of chemical enegy to kinetic energy is 53.1% efficient, how much energy will be available to impart to the bullet? Report in kJ with 3 singificant figures and use the following conversion factors:

1 cal = 4.184 J

1 grain = 0.0648 gram

HINT: kcal/kg = cal/g

Explanation / Answer

Q1.

MW = 341.5 g /mol

Hformation = -421.6 kJ/mol

1X --> 3CO(g) + 2CO2(g) + 7H2O(g)

Hcombustion = Hproducts - Hreactants

Hcombustion = 3*(-110.5 +2*-393.5 + 7*-241.8) - (-421.6) = -7348.7 kJ

this is per 1 mol

so

Hcomb = -7348.7 kJ/mol --> -7349 kJ/mol

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