Calculate the standard enthalpy of formation of CH₃OH. from the following data:
(i) CH₃OH(l) + 3/2 0₂ (g) ———-> CO₂ (g) + 2H₂0 (l); ∆_rH^– = – 726kj mol^-1
(ii) C(s) + 0₂(g) —————>C0₂ (g); ∆_cH^– = -393 kj mol^-1
(iii) H₂(g) + 1/20₂(g) —————->H₂0 (l); ∆_fH^– = -286 kj mol^-1

 For an isolated system∆U = 0; what will be ∆S? 

 For a reaction at 298 K
2A + B————->C
∆H = 40Q kj mot1 and AS = 0.2 kj Kr^-1 mol^-1.
At what temperature will the reaction become spontaneous considering ∆H and ∆S to be constant over the temperature range?

For the reaction; 2Cl(g) ———-> Cl₂(g); what will be the signs of ∆H and ∆S?

If ∆U = 0 how are q and w related to each other?

When is bond energy equal to bond dissociation energy ?

What is the enthalpy of formation of the most stable form of an element in its standard state?
 

Out of diamond and graphite, which has greater entropy

At what temperature entropy of a substance is zero?

From thermodynamic point of view, to which system the animals and plants belong

Predict the sign of ∆S for the following reaction heat
CaCO₃ (s) ———> CaO(s) + CO₂(g)