3 Nitroglycerine is used as an explosive.
The equation for the explosion reaction is:
4C3H5(NO3)3 ( l )
12CO2 ( g) 1 10H2O ( l ) 1 6N2 ( g) 1 O2 ( g)
a How many moles does the equation show for:
i nitroglycerine?
ii gas molecules produced?
b How many moles of gas molecules are obtained
from 1 mole of nitroglycerine?
c What is the total volume of gas (at rtp) obtained
from 1 mole of nitroglycerine?
d What is the mass of 1 mole of nitroglycerine?
(Ar : H 5 1, C 5 12, N 5 14, O 5 16.)
e What will be the total volume of gas (at rtp)
from exploding 1 kg of nitroglycerine?
f Using your answers above, try to explain why
nitroglycerine is used as an explosive.
idk broo 🙃 #Sikh #Akaal
a)
i) The equation shows that 4 moles of nitroglycerine (C3H5(NO3)3) are involved in the reaction.
ii) The equation shows that 12 moles of CO2, 10 moles of H2O, 6 moles of N2, and 1 mole of O2 are produced as gas molecules.
b) From the equation, we can see that for every 4 moles of nitroglycerine, 12 moles of CO2, 10 moles of H2O, 6 moles of N2, and 1 mole of O2 are produced. Therefore, for 1 mole of nitroglycerine, 12 + 10 + 6 + 1 = 29 moles of gas molecules are obtained.
c) At RTP (room temperature and pressure), 1 mole of any ideal gas occupies approximately 24 liters. Therefore, if we assume the volume of gases produced as ideal gases, then 1 mole of nitroglycerine would produce 29 moles of gas molecules, which would occupy 29 * 24 liters of volume.
d) To determine the mass of 1 mole of nitroglycerine, we need to calculate the molar mass. From the formula C3H5(NO3)3, we can calculate the molar mass as follows:
(3 * 12.01 g/mol) + (5 * 1.01 g/mol) + (3 * (14.01 * 3 + 16.00 * 3) g/mol) = 227.09 g/mol
Therefore, the mass of 1 mole of nitroglycerine is 227.09 grams.
e) To calculate the total volume of gas from exploding 1 kg of nitroglycerine, we first need to convert the mass of nitroglycerine to moles.
1 kg = 1000 grams
Number of moles = (1000 grams) / (227.09 g/mol) = 4.4 moles (approx.)
Since we know that 1 mole of nitroglycerine produces 29 moles of gas molecules, we can calculate the total volume of gas:
Total volume = (4.4 moles) * (29 * 24 liters/mole) = 3048.96 liters (approx.)
f) Nitroglycerine is used as an explosive because when it undergoes the given reaction, a large number of gas molecules are produced. The production of a large volume of gas results in a rapid expansion and release of energy, leading to a powerful explosion. The high number of gas molecules produced contributes to the explosive force of nitroglycerine.
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Very helpful
A
Part 1) 4
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B)
C)96dm