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1 ton of TNT can produce 4.6 x 109 J of energy. A chemist wants to...

1 ton of TNT can produce 4.6 x 109 J of energy. A chemist wants to know how to obtain this much energy from acetylene (C2H2) and Oxygen (O2). How much acetylene and Oxygen would be required? Provide the name and structure of the "TNT". Reaction between Acetylene and Oxygen: ΔH= -2510 KJ

Solutions

Expert Solution

Ans. Given,

            1 ton of TNT releases 4.6 x 109 J energy = 4.6 x 106 kJ.

TNT (2-methyl-1,3,5-trinitrobenzene)

# Balanced combustion of acetylene-

            2 C2H2 + 5 O2 ------------> 4 CO2 + 2 H2O                    ; dH = -2510 kJ

Note: Molar enthalpy of combustion of acetylene is -1255.57 kJ/mol. So, the value “2510 kJ” must be for two moles of acetylene as shown in above reaction.

# So, enthalpy of acetylene combustion = 2510 kJ/ 2 mol acetylene

Now,  

Amount of acetylene required = Energy from 1 ton TNT / enthalpy of acetylene

                                                = 4.6 x 106 kJ / (2510 kJ/ 2 mol acetylene)

                                                = 3.6653 x 103 mol acetylene.

According to the stoichiometry of balanced reaction, 1 mol acetylene reacts with 5 mol O2.

So,

            Required moles of O2 = (5 / 2) x required moles of acetylene

                                                = (5/ 2) x 3.6653 x 103 mol

                                                = 9.1633 x 103 mol

# Required mass of acetylene = Required moles x Molar mass

                                                = 3.6653 x 103 mol x (26.03788 g/ mol)

                                                = 9.8438 x 104 g

                                                = 98.438 kg

Required Mass of O2 = = 9.1633 x 103 mol x (31.9988 g/ mol)

                                                = 2.9322 x 105 g

                                                = 293.22 kg


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