The 3 equations we are working with are: Mg(s)+2HCl(aq)-->MgCl2(aq)+H2(g) delta
ID: 1074507 • Letter: T
Question
The 3 equations we are working with are:
Mg(s)+2HCl(aq)-->MgCl2(aq)+H2(g) delta H= -8.2x10^2 kJ
MgO(s)+2HCl(aq)--> MgCl2(aq)+H2O(l) delta H= -1.8x10^2 kJ
H2O(l)->H2O(g) delta H= 44kJ
Final equation we are trying to find is: Mg(s)+H20(G) --> MgO(s)+H20(g)
Create an Enthalpy diagram for the final reaction studied in today's lab experiment. nthalpy Mg (s) + H2O (g) MgO (s) + H2 (g) Show the enthalpy changes associated with the decomposition of the reactants into elements, and the recombination of the elements into the products, as well as the overall enthalpy change for the reaction. Reactants: Mgis)+H,g Use the Enthalpies of Formation values in the Appendix of your lecture textbook to calculate the appropriate H's.Explanation / Answer
Mg(s)+2HCl(aq)-->MgCl2(aq)+H2(g) delta H= -8.2x10^2 kJ ---------------> 1
MgO(s)+2HCl(aq)--> MgCl2(aq)+H2O(l) delta H= -1.8x10^2 kJ -------------------->2
H2O(l)->H2O(g) delta H= 44kJ ----------------------->3
substact 1 and 2 equations
Mg(s)+2HCl(aq)-->MgCl2(aq)+H2(g) delta H= -8.2x10^2 kJ
H2O(l) -------------------->H2O(g) delta H= 44kJ
(-) (-) (-)
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Mg(s) + H2O(g)+ 2HCl(aq) ----------------------> MgCl2(aq) + H2(g) +H2O(l) delt H = -864KJ -----------> 4
substact equation 4 and 2
Mg(s) + H2O(g)+ 2HCl(aq) ----------------------> MgCl2(aq) + H2(g) +H2O(l) delt H = -864KJ
MgO(s)+2HCl(aq)------------------------> MgCl2(aq)+H2O(l) delta H= -1.8x10^2 kJ
(-) (-) (-) (-)
------------------------------------------------------------------------------------------------------------------------------------------------
Mg(s) + H2O (g) ------------------------> MgO (s) + H2(g) delt H = -1044KJ >>>>>>answer
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