Nitroglycerin C3H5(NO3)2 is a common explosive which decomposes according to the equation.
4C3H5(NO3)2 - 12CO2 + 10H2O + O2 +6N2 ΔH= -5.720*10^3 KJ. Calculate the heat for the decomposition for the 10.6g of the Nitroglycerin.
The molar mass of nitroglycerin is 165. So the problem tells you that 5.72E3 kJ is released by 4*165 g. You have 10.6 g.
5.720E3 kJ x (10.2/4*165) = ?
To calculate the heat for the decomposition of 10.6g of Nitroglycerin (C3H5(NO3)2), we can use the concept of stoichiometry and the given balanced equation.
First, let's calculate the molar mass of Nitroglycerin:
C (Carbon) = 12.01 g/mol
H (Hydrogen) = 1.01 g/mol
N (Nitrogen) = 14.01 g/mol
O (Oxygen) = 16.00 g/mol
Molar mass of Nitroglycerin (C3H5(NO3)2) = (3 * C) + (5 * H) + (2 * (N + (3 * O)))
= (3 * 12.01) + (5 * 1.01) + (2 * (14.01 + (3 * 16.00)))
= 227.09 g/mol
Next, let's calculate the number of moles of Nitroglycerin used:
Number of moles = Mass / Molar mass
= 10.6g / 227.09 g/mol
= 0.0467 mol (rounded to four decimal places)
Now, we can use the balanced equation and the stoichiometry to calculate the amount of heat produced:
Given: 4C3H5(NO3)2 → 12CO2 + 10H2O + O2 + 6N2 ΔH = -5.720 * 10^3 KJ
From the equation, we can see that 4 moles of Nitroglycerin produce -5.720 * 10^3 KJ of heat.
To find the amount of heat produced by 0.0467 mol of Nitroglycerin, we can set up a proportion using the number of moles:
(0.0467 mol / 4 mol) = (x KJ / -5.720 * 10^3 KJ)
Cross-multiplying and solving for x:
x = (0.0467 mol * -5.720 * 10^3 KJ) / 4 mol
= -67.6 KJ
Therefore, the heat produced for the decomposition of 10.6g of Nitroglycerin is approximately -67.6 KJ. Note that the negative sign indicates the release of heat.