Calculate the heat of formation of acetic acid from the following data-a- Cs - O2g- CO2g- - H - -393-7 kJb- H2g -1-2O2g- H2Ol- - H - -285-8 kJc- CH3COOHl - 2O2g- 2CO2g - 2H2Ol- - H - -873-2 kJ

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

Heat of Formation

Calculate the...

Question

Calculate the heat of formation of acetic acid from the following data:
a. $C (s) + O_{2} (g) ⟶ C O_{2} (g)$ , $Δ H = - 393.7 k J$
b. $H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l)$ , $Δ H = - 285.8 k J$
c. $C H_{3} C O O H (l) + 2 O_{2} (g) ⟶ 2 C O_{2} (g) + 2 H_{2} O (l)$ , $Δ H = - 873.2 k J$

Δ_{f} H = - 485.8 k J m o l^{- 1}

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

Δ_{f} H = + 485.8 k J m o l^{- 1}

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

Δ_{f} H = - 1432.2 k J m o l^{- 1}

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

None of these

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

Open in App

Solution

Suggest Corrections

Similar questions

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

Δ H = - 94.0 K c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l)

Δ H = - 68.0 K c a l

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

Δ H = - 210.0 K c a l

C (s) + O_{2} (g) \to C O_{2} (g) Δ H = - 94.0 k c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l) Δ H = - 68.0 k c a l

C H_{3} C O O H (l) + 2 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l) Δ H = - 210.0 k c a l

6 C (s) + 3 H_{2} (g) ⟶ C_{6} H_{6} (l), Δ H = 49.0 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l), Δ H = - 285.8 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g), Δ H = - 389.3 k J

C H_{3} C O O H (l)

25^{\circ} C

C H_{3} C O O H (l) + 2 O_{2} (g) \to 2 C O_{2} + 2 H_{2} O (l); Δ H = - 208.34

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94.05

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

{C H}_{3} O H (l)

{C H}_{3} O H (l) + \frac{3}{2} O_{2} (g) ⟶ C O_{2} (g) + 2 H_{2} O (l); Δ H = - 726 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g); Δ H = - 394 k J

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

Join BYJU'S Learning Program