Calculate the heat of hydrogenation of C 2 H 2 to C 2 H 4 H 2 g -1-2 O 2 g - H 2 O l - - H -68-32 kcalC 2 H 2 g -1-2 O 2 g - 2 CO 2 g - H 2 O l - - H -310-61 kcalC 2 H 4 g -3-2 O 2 g - 2 CO 2 g -2 H 2 O l - - H -337-32 kcalA- - 51-46 kcalB- 41-46 calC- -41-46 kcalD- 81-46 kcal

The correct option is C 41.46 kcalGiven, nbsp; H_2(g)+1/2O_2(g)⇌ H_2O(l); Δ_f H= 68.32 kcal C_2H_2(g)+1/2O_2(g)⇌ 2CO_2(g)+H_2O(l); Δ_comb H= 310.61 kcal C_2 ...

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Standard XII

Chemistry

Heat of Reaction

Calculate the...

Question

Calculate the heat of hydrogenation of $C_{2} H_{2}$ to $C_{2} H_{4}$
$H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (l); Δ H = - 68.32 k c a l$
$C_{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ 2 C O_{2} (g) + H_{2} O (l); Δ H = - 310.61 k c a l$
$C_{2} H_{4} (g) + \frac{3}{2} O_{2} (g) ⇌ 2 C O_{2} (g) + 2 H_{2} O (l); Δ H = - 337.32 k c a l$

-51.46 kcal

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-41.46 kcal

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81.46 kcal

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41.46 cal

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Solution

The correct option is B -41.46 kcal
Given,
$H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (l); Δ_{f} H = - 68.32 k c a l$
$C_{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ 2 C O_{2} (g) + H_{2} O (l); Δ_{c o m b} H = - 310.61 k c a l$
$C_{2} H_{4} (g) + \frac{3}{2} O_{2} (g) ⇌ 2 C O_{2} (g) + H_{2} O (l); Δ_{c o m b} H = - 337.32 k c a l$
Heat of hydrogenation=heat of formation of water +heat of combustion of $C_{2} H_{2}$ - heat of combustion of $C_{2} H_{4}$
Heat of hydrogenation= $Δ_{f} H (H_{2} O)$ + $Δ_{c o m b} H (C_{2} H_{2} (g))$ - $Δ_{c o m b} H (C_{2} H_{4} (g))$
Heat of hydrogenation=(-68.32 - 310.61 + 337.32) kcal
Heat of hydrogenation= $- 41.61 k c a l$

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Similar questions

Q. Calculate the heat of hydrogenation of

C_{2} H_{2}

C_{2} H_{4}

H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ H_{2} O (l); Δ H = - 68.32 k c a l

C_{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ 2 C O_{2} (g) + H_{2} O (l); Δ H = - 310.61 k c a l

C_{2} H_{4} (g) + \frac{3}{2} O_{2} (g) ⇌ 2 C O_{2} (g) + 2 H_{2} O (l); Δ H = - 337.32 k c a l

Q. Calculate the heat of hydrogenation of

C_{2} H_{2}

C_{2} H_{4}

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); Δ H = - 68.32 k c a l

C_{2} H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ 2 C O_{2} (g) + H_{2} O (l); Δ H = - 310.61 k c a l

C_{2} H_{4} (g) + 3 O_{2} (g) ⟶ 2 C O_{2} (g) + H_{2} O (l); Δ H = - 337.32 k c a l

2 C (s) + 2 O_{2} (g) \to 2 C O_{2} (g), Δ H = - 787 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l), Δ H = - 286 k J

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) \to 2 C O_{2} (g) + H_{2} O (l), Δ H = - 1310 k J

From the above data, heat of formation of acetylene is:

Q. Given that:

2 C (s) + 2 O_{2} (g) ⟶ 2 C O_{2} (g); Δ H = - 787 k J . . . (i)

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (l); Δ H = - 286 k J . . . (i i)

C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) ⟶ 2 C O_{2} (g) + 3 H_{2} O (l) . . . . (i i i)

Δ H = - 1301 k J

Heat formation of acetylene is:

Q. Calculate the heat of formation of acetic acid from the following data:
a.

C (s) + O_{2} (g) ⟶ C O_{2} (g)

Δ H = - 393.7 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l)

Δ H = - 285.8 k J

C H_{3} C O O H (l) + 2 O_{2} (g) ⟶ 2 C O_{2} (g) + 2 H_{2} O (l)

Δ H = - 873.2 k J

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Heat of Reaction

Standard XII Chemistry

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Calculate the heat of hydrogenation of C2H2 to C2H4 H2(g)+12O2(g)⇌H2O(l);ΔH=−68.32 kcal C2H2(g)+12O2(g)⇌2CO2(g)+H2O(l);ΔH=−310.61 kcal C2H4(g)+32O2(g)⇌2CO2(g)+2H2O(l);ΔH=−337.32 kcal