Rewrite each equation below with the delta H value included with either the reactants or the products and identify the reaction as endothermic or exothermic.
A) H2(g) + O2 (g) - H2O (l);
DeltaH^0 = -285.83

B)2Mg(s) +O2(g) -2MgO(s); deltaH^0 =-1200kJ

Question

Rewrite each equation below with the delta H value included with either the reactants or the products and identify the reaction as endothermic or exothermic. 
A) H2(g) + O2 (g) -> H2O (l);
DeltaH^0 = -285.83

B)2Mg(s) +O2(g) ->2MgO(s); deltaH^0 =-1200kJ

anonymous · Answer

C)I2(s) -> i2(g) ; deltaH0 =62.4 kj

shiraz14 · Answer

Could you please scan your original question & upload it? There isn't enough information to state if this question requires you to draw an Energy Level diagram, etc?

kainui · Answer

$$\Delta H ^o = \Delta H_f ^o(products)-\Delta H_f ^o(reactants)$$ So you're given the standard enthalpy change, what is the enthalpy change for the products and reactants separately? Well, fortunately it's not that difficult. For pure substances such as O2 or H2 it is defined to be zero, so you can already write these down. The rest you can algebraically solve for! I suggest reading through this for more information. http://chemwiki.ucdavis.edu/Physical_Chemistry/Thermodynamics/State_Functions/Enthalpy/Standard_Enthalpy_Of_Formation