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The enthalpy of reaction does not depend...

The enthalpy of reaction does not depend upon:

A

the intermediate reaction steps

B

the temperature of initial and final state of the reaction

C

the physical states of reactants and products

D

use of different reactants for the formation of the same product

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(According to Hess' law)
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CENGAGE CHEMISTRY ENGLISH-THERMODYNAMICS-Archives (Subjective)
  1. The enthalpy of reaction does not depend upon:

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  2. The enthalpies for the following reactions (DeltaH^(Theta)) at 25^(@)C...

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  3. The standared enthalpies of formation at 298K for C C1(g), H(2)O(g), C...

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  4. Given that: i. C(s) + O(2)(g) rarr CO(2)(g) , DeltaH =- 94.05 kcal ...

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  5. The following statement is true only under some specific conditions. W...

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  6. The bond dissociation energies of gaseous H(2),Cl(2), and HCl are 100,...

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  7. The standard molar heat of formation of ethane, carbon dioxide and wat...

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  8. An intimate mixture of ferric oxide and aluminium is used as solid fue...

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  9. The enthalpy of combustion of H(2), cyclohexene (C(6)H(10)) and cycloh...

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  10. CsOH +HCI rarr CsCI +H(2)O, DeltaH =- 13.4 kcal mol^(-1)……….(i) CsOH...

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  11. Determine enthalpy change for, C(3)H(8(g))+H(2(g))rarr C(2)H(6(g))+C...

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  12. Compute the heat of formation of liquid methyl alcohol in kilojoule pe...

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  13. From the following data, calculate the enthalpy change for the combust...

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  14. The standard heat of formation values of SF(6)(g), S(g), and F(g) are ...

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  15. Show that the reaction CO(g) +(1//2)O(2)(g) rarr CO(2)(g) at 300K ...

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  16. A sample of argon gas at 1atm pressure and 27^(@)C expands reversibly ...

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  17. Determine the enthalpy of formation of B(2)H(6)(g) in kJ/mol of the fo...

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  18. The standart potential of the following cell is 0.23 at 15^(@)C and 0....

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  19. When 1pentyne (A) is treated with 4N alcoholic KOH at 175^(@)C, it is ...

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  20. Two moles of a perfect gas undergo the following processes: a. A rev...

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  21. C(v) values of He is always (3R)/(2) but C(v) values of H(2) is (3R)/(...

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