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Thursday, October 1, 2020

What are the "State functions or State variables" ?

State Functions or State Variables are the physical quantity having a definite value at a particular (present state) state and value is independent from the fact how the system achieved that state.

Mathematical Condition for a function to be a state function:-
There are three conditions that must be satisfied simultaneously for a function to be state      function.

(i) If ∆φ is a state function
        
    It means change in depends only on end states and not on the path which it followed       during the process.


(ii) If ∆φ is a state function
       



  It implies, in cyclic integral as the end states are same, so ∆φ value will be zero.

  (iii) If ∆φ = f(x, y) is a state function, Euler's reciprocity theorem must be satisfied.
           

                     If dz=0 then, are we sure that z = 0 state function ?


   "Change in state function (z) is fixed in between two states so ∆z is also
      a state function example ∆P,∆T,∆V,∆H= state function is a wrong statement"

The heats of solution of anhydrous CuSO4 and hydrated CuSO4.5H2O are 66.5 and 11.7 kJ mol1 respectively. Calculate the heat of hydration of CuSO4 to CuSO4.5H2O.

 


200 ml of KOH and 200 ml of HNO3 of same molarity are mixed together and liberated 3.426 kJ of heat. Determine the molarity of each solution.

 



Consider the chemical reaction at 300 K H2 (g) + Cl2 --> HCl(g) ΔH= -185KJ/mole calculate ΔU if 3 mole of H2 completely react with 3 mole of Cl2 (g) to form HCl.

 
                           H2 (g)+Cl2 -->  HCl(g) ΔH= -185KJ/mole
                                       Δng=0
                                   ΔH= ΔU+ ΔngRT
                                  ΔH= ΔU
                       ΔHR= -185 KJ/mole ,ΔUR= -185 KJ/mole
                       H2 (g)+Cl2 --> HCl(g) ΔH= -185KJ/mole
                         3 mole       3 mole
            Hence           ΔU= -185 X 3 KJ/Mole

What is the relation between change in enthalpy (dH ) and change in internal (dE) for combustion of methan ?

For the given reaction:

                        CH4(g) + 2O2(g) ---------> CO2(g) + 2H2O(l)
                                          dH = dE + dnRT
                            Dn = no. of mole of products - no. of moles of reactants = 1– 3 = –2
                                             DH = DE – 2RT