Consider the following thermochemical equation-C 2 H 4- H 2- C 2 H 6 - H 1-32-7 kcal1-3- butadiene -2 H 2- C 4 H 10 - H 2-40-2 kcalTherefore the magnitude of resonance energy of 1-3 -butadiene is- kcal

Given: C_2H_4+H_2→ C_2H_6; H_1= 32.7 kcal 1,3 butadiene+2H_2→ C_4H_10; H_2= 40.2 kcal The resonance energy of 1,3 butadiene is given as = (experimental value ...

You visited us 4 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Enthalpy

Consider the ...

Question

Consider the following thermochemical equation:
$C_{2} H_{4} + H_{2} \to C_{2} H_{6}; △ H_{1} = - 32.7 k c a l$
$1, 3 - b u t a d i e n e + 2 H_{2} \to C_{4} H_{10}; △ H_{2} = - 40.2 k c a l$
Therefore the magnitude of resonance energy of 1,3-butadiene is: $k c a l$

Open in App

Solution

Given:
$C_{2} H_{4} + H_{2} \to C_{2} H_{6}; △ H_{1} = - 32.7 k c a l$
$1, 3 - b u t a d i e n e + 2 H_{2} \to C_{4} H_{10}; △ H_{2} = - 40.2 k c a l$

The resonance energy of 1,3-butadiene is given as = (experimental value) - (calculated value)
$= △ H_{2} - 2 △ H_{1}$
$= - 40.2 - (2 \times - 32.7) = 25.2 k c a l$

Suggest Corrections

Similar questions

Q. If the enthalpy change for hydrogenation of ethylene is -132 kJ/mole and the enthalpy of formation of 1, 3-butadiene (g) and butane (g) are 115 kJ/mol and -140 kJ/mole respectively then calculate the magnitude of resonance energy of 1, 3-butadiene (in kJ)?

Q. If enthalpy change for hydrogenation of ethylene is

- 132

kJ/mole and enthalpy of formation

1, 3

-butadiene (g) and butane(g) are

115

kJ and

- 140

kJ/mole respectively then calculate resonance energy of

1, 3

-butadiene (in kJ)?

Q. Which of the following resonating structures of 1-methoxy-1,3-butadiene is least stable?

Q. From the following thermochemical equations:

C_{2} H_{4} \to C_{2} H_{6}; △ H = - 32.7 k c a l

C_{6} H_{6} + 3 H_{2} \to C_{6} H_{12}; △ H = - 49.2 k c a l

Calculate resonance energy of benzene.

Following are the thermochemical reactions:

H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H = - 68.39

kcal/mol

K + H_{2} O \to K O H (a q) + \frac{1}{2} H_{2}; Δ H = - 48.0

kcal/mol

K O H + H_{2} O \to K O H (a q); Δ H = - 14.0

kcal/mol

The heat of formation (in kcal/mol) of

K O H

is:

Join BYJU'S Learning Program

Consider the following thermochemical equation: C2H4+H2→C2H6; △H1=−32.7 kcal 1,3−butadiene+2H2→C4H10; △H2=−40.2 kcal Therefore the magnitude of resonance energy of 1,3-butadiene is: kcal

Given: C2H4+H2→C2H6; △H1=−32.7 kcal 1,3−butadiene+2H2→C4H10; △H2=−40.2 kcal The resonance energy of 1,3-butadiene is given as = (experimental value) - (calculated value) =△H2−2△H1 =−40.2−(2×−32.7)=25.2 kcal

Consider the following thermochemical equation:
$C_{2} H_{4} + H_{2} \to C_{2} H_{6}; △ H_{1} = - 32.7 k c a l$
$1, 3 - b u t a d i e n e + 2 H_{2} \to C_{4} H_{10}; △ H_{2} = - 40.2 k c a l$
Therefore the magnitude of resonance energy of 1,3-butadiene is: $k c a l$