Given- Cgraphite-O2g - CO2g- -rHo - -393-5 kJ mol-1 H2g-12O2g - H2Ol- -rHo - -285-8 kJ mol-1 CO2g-2H2Ol - CH4g - 2O2g- -rH6o - -890-3 kJ mol-1Based on the above thermochemical wquations- the value of DeltarHo at 298K for the reaction- Cgraphite - 2H2g - CH4g will be-

The correct option is A 78.8kJ mol^ 1 C + O_2 → CO_2 #160; #160; #160; #160; Δ H^o_r = 393.5 kJ/mol #160; #160; #8230; ...

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Bond Order and Enthalpy

Given, Cgra...

Question

Given, $C_{(g r a p h i t e} + O_{2} (g) \to C O_{2} (g); Δ_{r} H^{o} = - 393.5 k J m o l^{- 1}$
$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ_{r} H^{o} = - 285.8 k J m o l^{- 1}$
$C O_{2} (g) + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g); Δ^{r} H 6 o = + 890.3 k J m o l^{- 1}$
Based on the above thermochemical wquations, the value of $D e l t a_{r} H^{o}$ at $298 K$ for the reaction,
$C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)$ will be:

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

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+ 144.0 k J m o l^{- 1}

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+ 74.8 k J m o l^{- 1}

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

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C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g); Δ_{r} H^{o} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ_{r} H^{o} = - 285.8 k J m o l^{- 1}

C O_{2} (g) + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g); Δ_{r} H^{o} = + 890.3 k J m o l^{- 1}

Δ_{r} H^{o}

298 K

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

C_{(g r a p h i t e s)} + O_{2} (g) \to C O_{2} (g)

Δ_{r} H^{\circ} = - 393.5 k J m o l^{- 1}

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

Δ_{r} H^{\circ} = - 285.8 k J m o l^{- 2}

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

Δ_{r} H^{\circ} = + 890.3 k J m o l^{- 1}

Δ_{r} H^{\circ}

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g);

Δ_{f} H^{\circ} = - 393.5 k J m o l^{- 1}

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

Δ_{f} H^{\circ} = - 285.8 k J m o l^{- 1}

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

Δ_{f} H^{\circ} = + 890.3 k J m o l^{- 1}

Δ_{f} H^{\circ}

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

Determine $Δ U^{\circ}$ at 300 K for the following reaction using the listed enthalpies of reaction.

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

$C (g r a p h i t e) + \frac{1}{2} O_{2} (g) \to C O (g); Δ {H_{1}}^{\circ} = - 110.5 k J$

$C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g); Δ {H_{2}}^{\circ} = - 282.9 k J$

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H_{3}^{0} = - 285.8 k J$

$C (g r a p h i t e) + 2 H_{2} (g) \to C H_{4} (g); Δ H_{4}^{0} = - 74.8 k J$

Δ U^{o}

300 K

4 C O (g) + 8 H_{2} (g) ⟶ 3 {C H}_{4} (g) + {C O}_{2} (g) + 2 H_{2} O (l)

C_{(g r a p h i t e)} + 1 / 2 O_{2} (g) ⟶ C O (g); Δ {H_{1}}^{o} = - 110.5 k J

C O (g) + 1 / 2 O_{2} (g) ⟶ {C O}_{2} (g); Δ {H_{2}}^{o} = - 282.9 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l); Δ {H_{3}}^{o} = - 285.8 k J

C_{(g r a p h i t e)} + 2 H_{2} (g) ⟶ {C H}_{4} (g); Δ {H_{4}}^{o} = - 74.8 k J

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