The absolute value Delta H for the formation of compound A is calculated to be T

Question

The absolute value Delta H for the formation of compound A is calculated to be The formation of compound A is an process. -68 kcal/mole, exothermic +68 kcal/mole, endothermic -22 kcal/mole, endothermic -16 kcal/mole, exothermic +19 kcal/mole, endothermic The absolute value Delta H for the formation of compound B is calculated to be The formation of compound B is an process +86 kcal/mole, endothermic -31 kcal/mole, exothermic +30 kcal/mole, endothermic -28 kcal/mole, exothermic +62 kcal/mole, endothermic Which one of the molecules below has no net molecular dipole moment?

Explanation / Answer

32)

on reactant side:

1 C=C bond

3 C-C bond

1C=O bond

1 H-F bond

8 C-H bond

on product side:

1 C-F bond

1 C=O bond

4C-C bond

9 C-H bond

delta H = 1*H(C=C) +1*H(H-F) - H(C-C) - H (C-F) - 1*H(C-H)

= 146+ 136 - 90 - 115 -1*99

= -22 Kcal mol

It is exothermic since delta H is negative

Similarly please do the 2nd question

I am aallowed to answer only 1 question at a time

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