You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Enthalpy

CH2= CH2g + H...

Question

$C H_{2} = C H_{2} (g) + H_{2} (g) \to C H_{3} - C H_{3} (g)$ . The heat of reaction is: [bond energy of $C - C$ = $80 k c a l$ , $C = C$ $= 145 k c a l$ , $C - H$ $= 98 k c a l$ , $H - H$ $= 103 k c a l$ ]

- 12 k c a l

No worries! We‘ve got your back. Try BYJU‘S free classes today!

- 28 k c a l

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

- 41 k c a l

No worries! We‘ve got your back. Try BYJU‘S free classes today!

- 56 k c a l

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is D $- 28 k c a l$

Suggest Corrections

Similar questions

Q. Calculate the enthalpy of the following reaction:

H_{2} C = {C H}_{2} (g) + H_{2} (g) \to {C H}_{3} - {C H}_{3} (g)

The bond energies of

C - H, C - C, C = C

and

H - H

are

99, 83, 147

and

104

k c a l

respectively.

H_{2} C = C H_{2} (g) + H_{2} (g) ⟶ H_{3} C - C H_{3} (g)

The bond energy of

C - H, C - C, C = C, H - H

are

414, 347, 615, 435 k J m o l^{- 1}

respectively.

Enthalpy change of the above reaction is:

If at 298 K the bond energies of C - H, C - C, C=C and H - H bonds are respectively 414, 347, 615 and 435 kJ $m o l^{- 1}$ , the value of enthalpy change for the reaction
$C H_{2} = C H_{2} (g) + H_{2} (g) \to C H_{3} - C H_{3}$ is:

H_{2} C = C H_{2} (g) + H_{2} (g) \to H_{3} C - C H_{3} (g)

The bond energy of

C - H, C - C, C = C

and

H - H

are 414, 347, 615 and 435 kJ mol

^{- 1}

respectively.
If the enthalpy change of the above reaction is

x

kJ, then

\frac{- x}{25}

Calculate the enthalpy of the following reaction. $H_{2} C = C H_{2} (g) + H_{2} (g) \to C H_{3} - C H_{3} (g)$

The bond energies of C - H, C - C, C = C & H - H are 99, 83, 147 & 104 Kcal respectively.

Join BYJU'S Learning Program

CH2=CH2(g)+H2(g)→CH3−CH3(g). The heat of reaction is: [bond energy of C−C = 80kcal, C=C =145kcal, C−H =98kcal, H−H =103kcal]

The correct option is D −28kcal

$C H_{2} = C H_{2} (g) + H_{2} (g) \to C H_{3} - C H_{3} (g)$ . The heat of reaction is: [bond energy of $C - C$ = $80 k c a l$ , $C = C$ $= 145 k c a l$ , $C - H$ $= 98 k c a l$ , $H - H$ $= 103 k c a l$ ]

The correct option is D $- 28 k c a l$