Nitroglycerin, C3H5N3O9, is a shock sensitive liquid (density = 1.450 g/mL) that detonates by the reaction
4 C3H5N3O9(l) ® 10H2O(g) + O2(g) + 6N2(g) + 12CO2(g)
How many grams of N2 will be produced during the detonation of 2.813 L of nitroglycerin?
This is a simple stochiometric question
first convert to grams using density.
2813(mL)*1.45(g/mL) = 4078.85g
then convert this to moles of Nitroglycerin (requires molar mass)
(4078.85g)/(227.087g/mol)= 17.96mol of C3H5N3O9
Next, use your mol ratios to convert to moles of M2
(17.96mol(of NitroG.))*(6molN2/4molsC3H5N3O9)= 26.94mol N2
Next convert to grams of N2 using molar mass of N2 (28.02g/mol)
26.94mol*(28.02g/mol) = 754.93g N2 (rounded from 754.926)
if using correct sig figs then it would just be 754.9g N2
To calculate the number of grams of N2 produced during the detonation of nitroglycerin, we need to use the ideal gas law to determine the number of moles of N2 produced.
First, let's convert the volume of nitroglycerin from liters to milliliters:
2.813 L = 2813 mL
Next, let's find the number of moles of nitroglycerin. We can do this by using the density of nitroglycerin and its molecular weight.
The molecular weight of nitroglycerin (C3H5N3O9) is calculated as follows:
(3 x (12.01 g/mol)) + (5 x (1.01 g/mol)) + (3 x (14.01 g/mol)) + (9 x (16.00 g/mol)) = 227.09 g/mol
The mass of nitroglycerin can be calculated using the density:
Mass = Volume x Density
Mass = 2813 mL x 1.450 g/mL = 4082.65 g
The number of moles of nitroglycerin can be calculated using the mass and molecular weight:
Moles = Mass / Molecular Weight
Moles = 4082.65 g / 227.09 g/mol = 17.963 mol
Finally, we can use the balanced equation to calculate the number of moles of N2 produced. From the equation, we can see that 1 mole of nitroglycerin produces 6 moles of N2.
Moles of N2 = Moles of Nitroglycerin x (6 moles of N2 / 1 mole of Nitroglycerin)
Moles of N2 = 17.963 mol x (6 mol N2 / 1 mol Nitroglycerin) = 107.778 mol
To find the mass of N2 produced, we multiply the number of moles by its molecular weight.
Mass of N2 = Moles of N2 x Molecular Weight of N2
Mass of N2 = 107.778 mol x (2 x (14.01 g/mol)) = 3017.038 g
Therefore, during the detonation of 2.813 L of nitroglycerin, approximately 3017.038 grams of N2 will be produced.