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madam [21]
3 years ago
10

If a sample containing 2.50 ml of nitroglycerin (density=1.592g/ml) is detonated, how many total moles of gas are produced?

Chemistry
1 answer:
masya89 [10]3 years ago
3 0
<span>0.127 moles The formula for nitroglycerin is C3H5N3O9 so let's first calculate the molar mass of it. Carbon = 12.0107 Nitrogen = 14.0067 Hydrogen = 1.00794 Oxygen = 15.999 C3H5N3O9 = 3 * 12.0107 + 5 * 1.00794 + 3 * 14.0067 + 9 * 15.999 = 227.0829 Now calculate the number of moles of nitroglycerin you have by dividing the mass by the molar mass 2.50 ml * 1.592 g/ml / 227.0829 g/mol = 0.017527 mol The balanced formula for when nitroglycerin explodes is 4 C3H5N3O9 => 12 CO2 + 10 H2O + O2 + 6 N2 Since all of the products are gasses at the time of the explosion, there is a total of 29 moles of gas produced for every 4 moles of nitroglycerin Now multiply the number of moles of nitroglycerin by 29/4 0.017527 mol * 29/4 = 0.12707075 moles Round to 3 significant figures, giving 0.127 moles</span>
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Answer:

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Now we will reverse the reaction 3, multiply reaction 2 by 2  then adding all the equations, Using Hess's law:

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\Delta H_{formation}=\Delta H_1+2\times \Delta H_2+\Delta H_3

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\Delta H=-238.7kJ/mole

The standard enthalpy of formation of methanol is, -238.7 kJ/mole

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Answer:

Explanation:

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