Using bond energy data, calculate heat of formation of isoprene Given C−H, H−H, C−C, C=C and C(s)→ C(g) respectively as 98.8 kcal, 104 kcal, 83 kcal, 147 kcal, 171 kcal
5C(s)+4H2(g)→H2C=C|CH3−CH=CH2
-21 kcal
21 kcal
40 kcal
50 kcal
A
50 kcal
B
21 kcal
C
40 kcal
D
-21 kcal
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Q1
Using bond energy data, calculate heat of formation of isoprene Given C−H, H−H, C−C, C=C and C(s)→ C(g) respectively as 98.8 kcal, 104 kcal, 83 kcal, 147 kcal, 171 kcal
5C(s)+4H2(g)→H2C=C|CH3−CH=CH2
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Q2
Using bond energy data, calculate heat of formation of isoprene 5C(s) + 4H2(g) → H2C=C(CH3)-CH=CH2 Given C-H, H-H, C-C, C=C and C(s)→ C(g) respectively as 98.8 kcal, 104 kcal,83kcal,147 kcal, 171 kcal
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Q3
Using bond energy data, calculate heat of formation of isoprene Given $$ C-H,H-H,C-C,C=C $$ and $$ C(s) \rightarrow C(g) $$ respectively as $$ 98.8 kcal, 104 kcal, 83 kcal, 147 kcal,171 kcal$$
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Q4
Estimate the heat of formation of gaseous isoprene (H2C=CH3|c−H|C=CH2) from the following data;
Bond energies: C−H = 98.8 kcal/mole H−H = 104.0 kcal/mole C−C = 83.1 kcal/mole C=C = 147.0 kcal/moleHeat of sublimation of carbon (s) = 171.7 kcal per mole
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Q5
Calculate the enthalpy of the following reaction. H2C=CH2(g)+H2(g)→CH3−CH3(g)
The bond energies of C - H, C - C, C = C & H - H are 99, 83, 147 & 104 Kcal respectively.