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Comment on the thermodynamic stability o...

Comment on the thermodynamic stability of `NO_((g))`, given
`(1)/(2)N_(2)(g)+(1)/(2)O_(2)(g)rarrNO(g)" " : " " Delta_(r)H^(theta)=90 kJ mol^(-1)`
`NO(g)+(1)/(2)O_(2)(g)rarrNO_(2)(g)" ": " " Delta_(r)H^(theta)=-74 kJ mol^(-1)`

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In the formation of NO(g), heat is absorbed. Therefore, NO(g) has a higher heat content and is unstable. On the other hand, formation of `NO_2`(g) involves release of heat energy. Hence, `NO_2`(g) has a lower heat content and is stable. Its formation will take place.
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Comment on the thermodynamic stability of NO(g) , given 1/2N_(2)(g)+1/2O_(2)(g)rarr NO(g), Delta_(r)H^(Θ)=90 kJ mol^(-1) NO(g)+1/2O_(2)(g) rarr NO_(2)(g), Delta_(r)H^(Θ)=-74 kJ mol^(-1)

With the following infromations, determine standard Gibb's free energy of formation of N_(2)O_(4)(g). (1)/(2)N_(2)(g) + (1)/(2)O_(2)(g) rarr NO(g) " "DeltaG^(@)=86.6 KJ " ""….."(i) NO(g) + (1)/(2)O_(2)(g) rarr NO_(2)(g) " "DeltaG_(@) =34.82 KJ " ""....."(ii) 2NO_(2)(g) rarr N_(2)O_(4)(g) " G= 5.77 ""....."(iii)

Methanol can be prepared synthetically by heating carbon monoxide and hydrogen gases under pressure in the presence of a catalyst. The reaction is CO(g) +2H_(2)(g) rarr CH_(3)OH(l) Determine the enthalpy of this reaction by an appropriate combinantion of the following data: a. C_(("graphite")) +(1)/(2)O_(2)(g) rarr CO(g), DeltaH^(Theta)=- 110.5kJ mol^(-1) b. C_(("graphite")) +O_(2)(g) rarr CO_(2)(g), DeltaH^(Theta) =- 393.5 kJ mol^(-1) c. H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(l), DeltaH^(Theta) =- 285.9kJ mol^(-1) d. CH_(3)OH(l) +(3)/(2)O_(2)(g)rarr CO_(2)(g) +2H_(2)O(l),DeltaH^(Theta) =- 726.6 kJ mol^(-1)

Calculate the enthalpy of formation of Delta_(f)H for C_(2)H_(5)OH from tabulated data and its heat of combustion as represented by the following equaitons: i. H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g), DeltaH^(Theta) =- 241.8 kJ mol^(-1) ii. C(s) +O_(2)(g) rarr CO_(2)(g),DeltaH^(Theta) =- 393.5kJ mol^(-1) iii. C_(2)H_(5)OH (l) +3O_(2)(g) rarr 3H_(2)O(g) + 2CO_(2)(g), DeltaH^(Theta) =- 1234.7kJ mol^(-1)

On the basic of the following Delta_(r)G^(Theta) values at 1073K : S_(1)(s) +2O_(2)(g) rarr 2SO_(2)(g) Delta_(r)G^(Theta) =- 544 kJ mol^(-1) 2Zn(s) +O_(2)(g) rarr 2ZnO(s) Delta_(r)G^(Theta) =- 480 kJ mol^(-1) 2Zn(s) +S_(2)(s) rarr 2ZnS(s) Delta_(r)G^(Theta) =- 293 KJ mol^(-1) Show that roasting of zinc sulphide to zinc oxide is a spontaneous process.

On the basic of the following Delta_(r)G^(Theta) values at 1073K : S_(1)(s) +2O_(2)(g) rarr 2SO_(2)(g) Delta_(r)G^(Theta) =- 544 kJ mol^(-1) 2Zn(s) +O_(2)(g) rarr 2ZnO(s) Delta_(r)G^(Theta) =- 480 kJ mol^(-1) 2Zn(s) +S_(2)(s) rarr 2ZnS(s) Delta_(r)G^(Theta) =- 293 KJ mol^(-1) Show that roasting of zinc sulphide to zince oxide is a spontaneous process.

On the basic of thermochemical equations (I),(II)and (III), Find out which of the algebraic relationships given in options (a)to (d) is correct ? (I) C("graphite")+O_(2)(g)to CO_(2)(g), Delta_(r)H=XKJmol^(-1) (II) C("graphite")+(1)/(2)O_(2)(g)toCO(g), Delta_(r)H=yKJ mol^(-1) (III) CO(g)+(1)/(2)O_(2)(g)toCO_(2)(g), Delta_(r)H=zKJ mol^(-1)

Calculate the standard enthalpy of formation of CH_(3)OH(l) from the following data: CH_(3)OH(l)+3/2O_(2)(g) rarr CO_(2)(g)+2H_(2)O(l), …(i), Delta_(r)H_(1)^(Θ)=-726 kJ mol^(-1) C(g)+O_(2)(g) rarr CO_(2)(g), …(ii), Delta_(c )H_(2)^(Θ)=-393 kJ mol^(-1) H_(2)(g)+1/2O_(2)(g) rarr H_(2)O(l), ...(iii), Delta_(f)H_(3)^(Θ)=-286 kJ mol^(-1)

With the help of thermochemical equations given below, determine Delta_(r )H^(Θ) at 298 K for the following reaction: C("graphite")+2H_(2)(g) rarr CH_(4)(g),Delta_(r )H^(Θ) = ? C("graphite")+O_(2)(g) rarr CH_(2)(g), Delta_(r )H^(Θ) = -393.5 kJ mol^(-1) ...(1) H_(2)(g) +1//2O_(2)(g) rarr H_(2)O(l) , Delta_(r )H^(Θ) = -285.8 kJ mol^(-1) ...(2) CO_2(2)(g)+2H_(2)O(l) rarr CH_(4)(g)+2O_(2)(g) , Delta_(r )H^(Θ) = +890.3 kJ mol^(-1) ...(3)

At 25^(@)C , the following heat of formations are given: {:("Compound",SO_(2)(g),H_(2)O(l),,),(Delta_(f)H^(Theta)kJmol^(-1),-296.0,-285.0,,):} For the reactions at 25^(@)C , 2H_(2)S(g) +Fe(s) rarr FeS_(2)(s) +2H_(2)(g), DeltaH^(Theta) =- 137 kJ mool^(-1) H_(2)S(g) +(3)/(2)O_(2)(g) rarr H_(2)O(l) +So_(2)(g),DeltaH^(Theta) =- 562kJ mol^(-1) Calculate the heat of formation of H_(2)S(g) and FeS_(2)(g) at 25^(@)C .

ICSE-CHEMICAL THERMODYNAMICS -NCERT TEXT-BOOK. EXERCISES
  1. The enthalpies of all elements in their standard states are

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  2. DeltaU^@ of combustion of methane is -X kJ mol^(-1). The value of Delt...

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  3. The enthalpy of combustion of methane, graphite and dihydrogen at 298 ...

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  4. A reaction A + B toC + D + q is found to have a positive entropy chang...

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  5. In a process, 701 J of heat is absorbed by a system and 394 J of work ...

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  6. The reaction of cyanamide, NH(2)CN (s), with dioxygen was carried out ...

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  7. Calculate the number of kJ of heat necessary to raise the temperature ...

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  8. The enthalpy change on freezing of 1 mol of water at 5^(@)C to ice at ...

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  9. Enthalpy of combustion of carbon to CO2 is -393.5 kJ mol^(-1) Calcu...

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  10. Enthalpies of formation of CO(g).CO(2)(g) and N(2)O(4) are -110,-393,8...

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  11. Given N(2)(g)+3H(2)(g)rarr2NH(3)(g),Delta(r)H^(Ө)= -92.4 kJ mol^(-1...

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  12. Calculate the standard enthalpy of formation of CH(3)OH(l) from the fo...

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  13. Calculate the enthalpy change for the process C CI(4)(g)rarrC(g)+4C...

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  14. For an isolated system, DeltaU=0, what will be Delta S?

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  15. For the reaction at 298 K, 2A + B to C DeltaH=400 KJ mol^(-1) an...

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  16. For the reaction, 2Cl(g) to Cl2(g), what are the signs of DeltaH and D...

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  17. For the reaction 2A(g)+B(g)rarr2D(g) DeltaU^(theta)=-10.55 KJ and ...

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  18. The equilibrium constant for a reaction is 10. What will be the value ...

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  19. Comment on the thermodynamic stability of NO((g)), given (1)/(2)N(2)...

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  20. Calculate the entropy change in surroundings when 1.00 mole of H2O(l) ...

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