Diborane is a potential rocket fuel which undergoes combustion according to the reaction B2H6g - 3O2g - B2O3s - 3H2Og From the following data- calculate the enthalpy change for the combustion of diborane-

B _ 2 H _ 6 ( g ) +3 O _ 2 ( g ) ⟶ B _ 2 O _ 3 ( s ) +3 H _ 2 O( g ) enthalpy change, #160; Δ H=[ Δ H _ B _ 3 O _ 3 ( s ) #160; +3Δ H _ H _ 2 O( ...

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

Enthalpy of Combustion

Diborane is a...

Question

Diborane is a potential rocket fuel which undergoes combustion according to the reaction $B_{2} H_{6} (g) + 3 O_{2} (g) \to B_{2} O_{3} (s) + 3 H_{2} O (g)$ From the following data, calculate the enthalpy change for the combustion of diborane.
$2 B (s) + (3 / 2) O_{2} (g) \to B_{2} O_{3} (s)$ $Δ H = 1273 K J / m o l$
$H_{2} (g) + (1 / 2) O_{2} (g) \to H_{2} O (1)$ $Δ H = - 286 K J / m o l$
$H_{2} O (l) \to H_{2} O (g)$ $Δ H s = 44 K J / m o l$
$2 B (s) + 3 H_{2} (g) \to B_{2} H_{6} (g)$ $Δ H = 36 K J / m o l$

Open in App

Solution

Suggest Corrections

Similar questions

B_{2} H_{6 (g)} + 3 O_{2 (g)} \to B_{2} O_{3 (s)} + 3 H_{2} O (g)

2 B (s) + (3 / 2) O_{2 (g)} \to B_{2} O_{3 (s)}

Δ H = - 1273 k J m o l^{- 1}

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

Δ H = - 286 k J m o l^{- 1}

H_{2} O_{(} 1) \to H_{2} O_{(} g)

Δ H = 44 k J m o l^{- 1}

2 B (s) + 3 H_{2 (g)} \to B_{2} H_{6 (g)}

Δ H = 36 K J m o l^{- 1}

2 B (s) + \frac{3}{2} O_2 (g) \to B_{2} O_{3} (s .)

Δ H = - 1273 k j

H_2 (g) + \frac{1}{2} O_2 (g) \to H_2 O (l)

Δ H = - 286 k j

H_{2} O (l) \to H_{2} O (g)

Δ H = 44 k j

2 B (s) + 3 H_{2} (g) \to B_{2} H_{6} (g)

Δ H = 365 k j

B_{2} H_{6} (g) + 3 O_{2} (g) B_{2} O_{3} (s) + 3 H_{2} O (g)

Δ H = ?

6 C (s) + 3 H_{2} (g) \to C_{6} H_{6} (l); Δ H = + 45.9 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H = - 285.9 k J

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 k J

{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

C H_{3} O H (l)

C H_{3} O H (l) + \frac{3}{2} O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l); △_{r} H^{⊖} = - 726 k J

C (s) + O_{2} (g) \to C O_{2} (g), Δ H = - 394 k J

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

Join BYJU'S Learning Program