Given the equation 2mg(s) + o2(g) → 2mgo(s) + 72.3 kj, how much heat is involved in the production of 5.0 mol of mgo?

The Balance Chemical equation is as follow,

                       2 Mg (s) + O₂(g) → 2 MgO(s) + 72.3 kJ

According to this equation,

             2 Moles of MgO formation involved  =  72.3 kJ of Heat
So,
         5 Moles of MgO formation will involve  =  X kJ of Heat

Solving for X,
                           X  =  (5 Moles × 72.3 kJ) ÷ 2 Moles

                           X  =  180.75 kJ of Heat

Hi. where is the graph?

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