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From the equation H=W+PV, explain what H...

From the equation H=W+PV, explain what H is a state function.

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CHHAYA PUBLICATION-CHEMICAL THERMODYNAMICS-WARM UP EXERCISE
  1. For an ideal gas, the isothermal free expansion and adiabatic free exp...

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  2. For chemical changes, why is the change in enthalpy more useful than t...

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  3. From the equation H=W+PV, explain what H is a state function.

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  4. From the definition of enthalpy show that for n mol of an ideal gas H=...

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  5. Prove that for an ideal gas undergoing an isothermal change, DeltaH=0.

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  6. Under what conditions are (i) DeltaU=q(V)& (ii) DeltaH=q(P) ?

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  7. Why is the heat capacity a path-dependent quantity?

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  8. Heat required to raise the temperatuer of 1 mol of a gas by 1^(@)C is ...

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  9. Why is the molar heat capacity at constant pressure greater than that ...

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  10. c(P)-c(V)=xJ*g^(-1)*K^(-1) and C(P,m)-C(V,m)=Xj*mol^(-1)*K^(-1) for an...

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  11. Why is the sign of DeltaH negative for an exothermic reaction and why ...

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  12. A 0.5 mol sample of H(2)(g) reacts with a 0.5 mol sample of Cl(2)(g) t...

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  13. A 1 mol sample of N(2)(g) reacts with 1 mol of O(2)(g) to form 2 mol o...

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  14. Identify the exothermic and endothermic changes: (i) NO(g)+(1)/(2)O(...

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  15. Write down the thermochemical equations for the following reactions: ...

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  16. H(2)(g)+(1)/(2)O(2)(g)toH(2)O(l),DeltaH=-285.8kJ. What will be the val...

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  17. Show that the difference between the heat of reactionn at constant pre...

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  18. What do you mean by the standard state of a substance? Is 25^(@)C the ...

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  19. Why is the concept of standard state necessary? What do you mean by th...

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  20. Mention the standard states of the following elements at 25^(@)C and 1...

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