Ready heat meals contain a self contained heat source. The reaction is Mg(s)+2H2

Question

Ready heat meals contain a self contained heat source. The reaction is Mg(s)+2H2O -> Mg(OH)2+H2 Calculate delta H^o , delta S^o, Delta g^o and K. Is the reaction spontaneous and why does the S value make sense Ready heat meals contain a self contained heat source. The reaction is Mg(s)+2H2O -> Mg(OH)2+H2 Calculate delta H^o , delta S^o, Delta g^o and K. Is the reaction spontaneous and why does the S value make sense Mg(s)+2H2O -> Mg(OH)2+H2 Calculate delta H^o , delta S^o, Delta g^o and K. Is the reaction spontaneous and why does the S value make sense

Explanation / Answer

We will need the next data:

Enthalpy Data (kJ/mol)

Hf Mg(s) = 0

Hf H2O(l) =

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