Asked by Shane
(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.
Answers
Answered by
DrBob222
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.
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.
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