When 2 mol of solid magnesium mg combines with 1 mole of oxygen gas 2 mol of solid magnesium oxide is formed and 1204 kj of heat is released write the thermochemical equation for the combustion reaction?

In a combustion reaction, element or molecule reaction with oxygen to form corresponding oxide.

In present case, 2 mol of solid magnesium mg combines with 1 mole of oxygen gas 2 mol of solid magnesium oxide is formed and 1204 kj of heat is released. The balanced thermochemical equation for the combustion reaction is 

2Mg    +    O2    →      2 MgO     +   1204 kJ

here, 1204 kJ is the energy liberated by the system during the reaction. Liberation of energy suggest the it is an exothermic reaction and the resultant product formed is thermodynamically more stable than reactant. 

Because electrons have negligible mass, to account for the mass of the isotope, there must be 16 neutrons, 16 neutrally charged, massive, fundamental particles present in the sulfur nucleus. and thus finally, if we have the 32s2− ion, there are 18 electrons, 16 protons, and 16 neutrons.