(1) Use the thermodynamic values to (a) deduce the enthalpy change of each reaction (b)state if the reaction is exothermic,or endothermic,and also how much energy is released or absorbed. For thi reactions; (1) NH4NO3 (s)------N2 (g) + 2H2O (l) (2) 4Zn (s) + 9HNO3 (aq)-------4Zn(NO3)2 (aq) + NH3 (g) 3H20 (l) (2) Predict the shift in equilibrium,if additional energy is added to the chemical reactions (1) and (2) above separately.

Question

(1) Use the thermodynamic values to (a) deduce the enthalpy change of each reaction (b)state if the reaction is exothermic,or endothermic,and also how much energy is released or absorbed. For thi reactions;                                                      (1) NH4NO3 (s)------>N2 (g) + 2H2O (l)    (2) 4Zn (s) + 9HNO3 (aq)------->4Zn(NO3)2 (aq) + NH3 (g) 3H20 (l)                     (2) Predict the shift in equilibrium,if additional energy is added to the chemical reactions (1) and (2) above separately.

DrBob222 · Answer

You have a book here.
dHrxn = (n*dHproducts) - (n*dH reactants). You can find dH for substances probably in a table in your text/notes.

If dHrxn is - it is exothermic
If dHrxn is + it is endothermic.

Adding heat to an exothermic rxn shifts it to the products.