In: Chemistry
Consider these reactions where M represents a generic metal:
2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta H1 = -569kj
HCl(g) ----> HCl(aq) DeltaH2 = -74.8
H2(g) + Cl2(g) ----> 2HCl(g) Delta H3 = -1845kj
MCl3(s) ----> MCl3(aq) Delta H4 = -405kj
Use the above information to determine the enthalpy of the following reaction:
2M(s) + 3Cl2(g) ----> 2MCl3(s) What is Delta H for this reaction?
notes:
use hess laws for enthalpy changes
note that we need
2M(s) in the left, so eqn 1 remains the same
we need to cancel HCl(aq) so, we need to multiply eqn 2 by (6)
then
2M(s) + 6HCl(aq) ---->2MCl3(aq) + 3H2(g) Delta H1 = -569
6HCl(g) ----> 6HCl(aq) DeltaH2 = -74.8*6 = -448.8
Add both equations
2M(s) + 6HCl(aq)+6HCl(g) ---->2MCl3(aq) + 3H2(g) + 6HCl(aq) dHRxn = -569+-448.8 = -1017.8
cancel common terms
2M(s) +6HCl(g) ---->2MCl3(aq) + 3H2(g) Hrxn = -1017.8
Now, we need to ancel HCl and H2
Eqn 3 must be mutiplied by 3
2M(s) +6HCl(g) ---->2MCl3(aq) + 3H2(g) Hrxn = -1017.8
3H2(g) + 3Cl2(g) ----> 6HCl(g) Delta H3 = -1845*3 = -5535
add both equations
2M(s) +6HCl(g) +3H2(g) + 3Cl2(g) ----->2MCl3(aq) + 3H2(g) +6HCl(g) Hrxn = -1017.8+ -5535 = -6552.8
cancel common terms
2M(s) + 3Cl2(g) ----->2MCl3(aq) Hrxn = = -6552.8
Now, we need MCl3 in solid state not aquous so...
from equation 4, invert it and mutiply by 2
2M(s) + 3Cl2(g) ----->2MCl3(aq) Hrxn = = -6552.8
2MCl3(aq) ---->2MCl3(s) Delta H4 = +405*2 = 810
Add both
2M(s) + 3Cl2(g)+2MCl3(aq)----->2MCl3(aq) +2MCl3(s) Hrxn = = -6552.8+810
cancel common terms
2M(s) + 3Cl2(g)----->2MCl3(s) Hrxn = = -5742.8 kJ
which is what we wanted