Entropy change and heat for reaction A+B→D with temperature-dependent heat capacities

[quietrain]

Homework Statement

if i have reaction A + B --> D

if i produce 1 mol of D, what is the entropy change?
how much heat is transferred?
is this exothermic or endothermic?

Homework Equations

reaction carried out at T = 300K,

molar heat capacities(constant Pressure),

C_A = 5sqrt(T)
C_B = 8sqrt(T)
C_D = 12sqrt(T)

The Attempt at a Solution

change in s = ∫ dQ / T right?

so ∫ C_p dT /T

but what are my limits for my Temperature?

is it right to say since they equalize at some temperature, i don't need to know my upper bound?

so i take C_D - (C_B + C_A) to get -1sqrt(T) ?

so Q = C_pT = -1(sqrt300) * 300

so since it is -ve, heat is released, and reaction is exothermic?

thanks

 

[Amok]

Are you sure this is all the data there is?

 

[quietrain]

er yes. that's all .

i read this lecture notes from MIT 5.60

it says dH/dT at constant pressure gives heat capacity at constant pressure

so i can sub into this equation?

∆C_p= ∑vC_p (products) - ∑vC_p (reactants)

where v is the stoichiometric coefficients

http://ocw.mit.edu/courses/chemistr...s-spring-2008/lecture-notes/5_60_lecture6.pdf
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