Answer:
A) -277.6 KJ/mol
Explanation:
The enthalpy data for first equation is not given but it should be somewhere around ΔH = –1367 kJ/mol.
So, Basically you want to rearrange the given three equations to match the equation they want you to have. To get the final equation, reverse reaction first reaction (turn its value into positive), multiply second equation by 2, multiply third equation by 3 and you add em all up:
You get 1367 + (2* -393.5) + (3 * -285.8) ~ -277.6 KJ/mol
