Question

Enthalpy Diagram for Mg(s)+H2O(g)--> MgO(s)+H2(g)

Answer 1

Not sure how to start- i have the enthalpies of formation though

Answer 2

Enthalpy of formation for H2 and Mg should be zero because they are both naturally occurring

Answer 3

Yes i have the enthalpies of formation, but not sure how to actually construct the diagram

Answer 4

Mg- 0
H2- 0
H2O- -241.8
MgO- -601.8

Answer 5

Subtract [Products - reactants] and if you get a number that's greater than zero it's endothermic if it's less than zero it's exptiermic. Then we will focus on constructing the diagram

Answer 6

Alright i did -601.8+241.8= -387

Answer 7

The zeros cancel out and the double negative becomes a positive

Answer 8

So its a - number= exothermic

Answer 9

So it's exothermic . That means that the products are at a lower energy than the reactants.' M

Answer 10

Yep- so do i start with the reactants?

Answer 11

So from here you need to construct your graph Y a is is energy X axis is reaction progress

Answer 12

Yeah so you would then put the enthLpy of formation of the reactants draw this as a horizontal line and do the same for the products