You visited us 2 times! Enjoying our articles? Unlock Full Access!

Heat of Formation

The heat of f...

Question

The heat of formation of $C O_{2} (g)$ is -394 kJ/mole and that of $H_{2} O (l)$ is -286 kJ/mole. The heat of combustion of $C_{2} H_{4}$ is -1412 kJ/mole. What is the heat of formation of $C_{2} H_{4}$ ?

$C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l)$

+ 1360

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

- 108

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

+ 52

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

+ 108

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

Open in App

Solution

The correct option is C $+ 52$
Heat of a reaction = heat of formation of products - heat of formation of reactants
here,

$C_{2} H_{4} + 3 O_{2} \to 2 C O_{2} + 2 H_{2} O$

so heat of reaction :

$- 1412 = (- 2 \times 394) - (286 \times 2$ ) - heat of formation of $C_{2} H_{4}$ - 0

heat of formation of $C_{2} H_{4}$ = $52 k J / m o l$

Suggest Corrections

Similar questions

C O_{2} (g)

H_{2} O (l)

- 394

- 285.8

C_{2} H_{2} (g)

2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 C O_{2} (g) + 2 H_{2} O (l)

Δ H^{o} = - 2601

C (s) + O_{2} (g) \to C O_{2} (g)

Δ H = - 394

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 1058

C_{3} H_{6}

^{- 1}

C O_{2} (g)

H_{2} O (l)

^{- 1}

^{- 1}

C_{3} H_{6}

C O_{2} (g)

H_{2} O (I)

C_{3} H_{8} (g)

C_{3} H_{8} (g) + 5 O_{2} (g) \to 3 C O_{2} (g) + 4 H_{2} O (l)

Δ H_{r x n}^{\circ} = - 2221.6 k J

C O

{m o l}^{- 1}

C O_{2}

{m o l}^{- 1}

Join BYJU'S Learning Program