Ch4(g) + h2o(g) 3h2(g) + co(g) enthalpy of formation of CH4
1 answer:
You might be interested in
The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction.
Bond energy has been defined as the chemical energy possessed by the bonds in the chemical structure. The energy has been conserved in the chemical reaction.
<h3>Is the reaction endothermic or exothermic?</h3>In the reaction in which bond energy of the reactant has been higher than the product, it has been an exothermic reaction.
In the reaction in which the bond energy of the product is higher than the reactant, it has been an endothermic reaction.
In the given reaction
The bond energies of reactant has been:
- H-C bond = 413 kJ/mol
- C-C bond = 347 kJ/mol
The total bond energy of the reactant has been:
The total bond energy of the reactant has been 2,825 kJ/mol.
The bond energies of product has been:
- H-C = 413 kJ/mol
- C=C = 614 kJ/mol
- H-H = 432 kJ/mol
The total bond energy of the product has been:
The total bond energy of the product has been 2,698 kJ/mol.
The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction, as energy can neither be created nor be destroyed. It has been conserved in the chemical reaction.
Learn more about exothermic reaction, here:
Explanation:
Dehydrohalogenation reactions occurs as elimination reactions through the following mechanism:
Step 1: A strong base(usually KOH) removes a slightly acidic hydrogen proton from the alkyl halide.
Step 2: The electrons from the broken hydrogen‐carbon bond are attracted toward the slightly positive carbon (carbocation) atom attached to the chlorine atom. As these electrons approach the second carbon, the halogen atom breaks free.
However, elimination will be slower in the exit of Hydrogen atom at the C2 and C3 because of the steric hindrance by the methyl group.
Elimination of the hydrogen from the methyl group is easier.
Thus, the major product will A
