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

Enthalpy of Combustion

Δ U0 of combu...

Question

$Δ U^{0}$ of combustion of $C H_{4_{(} g)}$ at certain temperature is -393 kJ $m o l^{- 1}$ . The value of $Δ H^{0}$ is:

zero

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

Δ U^{0}

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

Δ U^{0}

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

equal to

Δ U^{0}

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

Open in App

Solution

The correct option is A < $Δ U^{0}$
The balanced equation for combustion of methane is:

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

Here, $Δ n_{g} = 1 - 3 = - 2$

$Δ H^{0} = Δ U^{0} + Δ n_{g} R T$

$Δ H^{0} = - 393 - 2 R T$

$∴ Δ H^{0} < Δ U^{0}$

Suggest Corrections

Similar questions

Δ H^{0}

X_{(g)} + Y_{(g)} ⇌ Z_{(g)}

Δ U^{0}

227^{o} C

R = 2 c a l {m o l}^{- 1} K^{- 1}

Δ H^{0}

X_{(g)} + Y_{(g)} ⇌ Z (g)

- 4.6

Δ U^{0}

227^{0}

(R = 2 c a l . m o l^{- 1} K^{- 1})

Δ U

C H_{4} (g)

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

- 393 k J m o l^{- 1}

Δ H

Δ U

C H_{4} (g)

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

- 393 k J m o l^{- 1}

Δ H

∆U° of combustion of CH4 (g)at certain temperature is -393kj/ mol.Then value of ∆H° is

1)0

2)<∆U°

3)>∆U°

4)=∆U°

Join BYJU'S Learning Program