The explosive nitroglycerin (c3h5n3o9) decomposes rapidly upon ignition or sudden impact according to the following balanced equation: 4 c3h5n3o9 (l) → 12 co2 (g) + 10 h2o (g) + 6 n2 (g) + o2 (g) δrxnho = −5678 kj calculate the standard enthalpy of formation (δfho) for nitroglycerin. the enthalpy of formation of co2 (g) is -393.5 kj/mol. the enthalpy of formation of h2o (g) is -241.8 kj/mol.

The for in the reaction is -365.5 kJ/mol.

Explanation:

Enthalpy change of a reaction is defined as the difference in enthalpy of all the products and the reactants each multiplied with their respective number of moles. The equation that is used to calculate the enthalpy change of a reaction is:

For the given chemical reaction:

The equation for the enthalpy change of the above reaction is:

We are given:

Putting values in above equation, we get:

Hence, the for in the reaction is -365.5 kJ/mol.

is has three carbons, so the answer is propylamine.

meth-

eth-

prop-

but-

pent-

hex-

hept-

oct-

non-

explanation:

b. th3 n4zc4 pl4t3 15 c0nv3rg1ng w1th the s0uth 4m3ric4n pl4t3.