U3-3-3 - Hess's Law Flashcards
Part of the Chemical Energy topic from Unit 3 of Higher Chemistry, Chemistry in Society
State Hess’s law
The enthalpy change for a chemical reaction is independent of the route taken.
Overall ∆H is the same regardless of any intermediates formed
∆H1 = …
∆H1 = ∆H2 + ∆H3
In the type of diagram shown, how do you know if the sign (+ or −) for ∆H should be reversed or not?
Going in same direction as arrow (e.g. W to Z) - sign stays as is
Going in opposite direction to arrow (e.g. Z to W) - sign reversed
What change needs to be applied to the highlighted equation’s ∆H to calculate enthalpy change for the top reaction?
x3
(3 moles of C in target equation)
so -394 x 3
What change needs to be applied to the highlighted equation’s ∆H to calculate enthalpy change for the top reaction?
x2
(2 moles of H2 in target equation)
so -286 x 2
What change needs to be applied to the highlighted equation’s ∆H to calculate enthalpy change for the top reaction?
reverse
(C3H4 is a product in target equation)
so +1939