Hey =) I am just gonna perform my better to help you and this is what My spouse and i came up with.... I came across out how to get the mixture of Mg + 1/2 O2 ---> MgO...
The only thing is that I missed the (delta) H pertaining to the target method. I believe you could find it making use of the appendix of your book ( assuming they desire you to find the typical Enthalpies of Formation intended for the other formulas ).... For my own rference to them through this answer, We substituted the values with variables....
To look for Mg + 1/2 T-MOBILE --> MgO,
(1) Magnesium + 2HCl --> H2 + MgCl2 (delta) H = X
(2) MgO + 2HCl --> WATER + MgCl2 (delta) They would = Sumado a
(3) H2 + .5 O2 --> H2O (delta) H = -285. eight KJ
You understand you already need the Mg and the .5 O2 on the left and the MgO on the proper side with the equasion.... I saw quickly the Mg and 1/2 UNITED KINGDOM are already on the left hand side but the MgO in picture (2) was on the left. Therefore , I switched it around. I ended with
(1) Mg + 2HCl --> H2 & MgCl2 (delta) H sama dengan X
(2) H2O + MgCl2 --> MgO & 2HCl (delta) H = -Y
(3) H2 & 1/2 T-MOBILE --> H2O (delta) H = -285. 8 KJ
Basically, only the second picture changed and the Y is now negative trigger u changed the products and reactants....
My spouse and i tried doing work it below and incorporating them. Everything proceeded to cancel out apart from the Mg, 1/2O2 and MgO =) Hope you understood all that!
OH and I'm sure you know how to find the Normal Enthalpy of Formation pertaining to an equasion... But in case you don't it can.... [Sum Products] - [ Sum Reactants] -- Just like I explained, all enthalpies should be in the back of the book. Be sure if you're careful to mind the state of the chemical. Particular substances like Water exist as a liquid and a gas by room temperatures. Therefore , make sure you look at the GAS Enthalpy for gas as well as the LIQUID enthalpy for the liquid