Given that-i- Cgraphite - O2g- CO2g- - H - -393-7 kJii- Cdiamond- Cgraphite- - H - -2-1 kJcalculate - H for burning of diamond to CO2-

The correct option is A Δ H = 395.8 kJ Given that:i. #160; C(graphite) + O_2(g)⟶ CO_2(g); Δ H = 393.7 kJ ii. #160; C(diamond)⟶ C(graphite); ...

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Enthalpy of Combustion

Given that:i....

Question

Given that:
i. $C (g r a p h i t e) + O_{2} (g) ⟶ C O_{2} (g); Δ H = - 393.7 k J$
ii. $C (d i a m o n d) ⟶ C (g r a p h i t e); Δ H = - 2.1 k J$
calculate $Δ H$ for burning of diamond to $C O_{2}$ .

Δ H = - 395.8 k J

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Δ H = - 152.4 k J

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Δ H = + 395.8 k J

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None of these

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C_{(g r a p h i t e)} + O_{2 (g)} \to C O_{2 (g)}; Δ H = - 393.7 k J

C_{(d i a m o n d)} \to C_{(g r a p h i t e)}; Δ H = - 2.1 k J

Calculate $Δ H$ for $C_{(g r a p h i t e)} \to C_{d i a m o n d}$ from the following data:

i) $C (g r a p h i t e) + O_{2} \to C O_{2} (g), Δ H = - 94 K c a l$

ii) $C (d i a m o n d) + O_{2} \to C O_{2} (g), Δ H = - 68 K c a l$

Δ H

C (d i a m o n d) + O_{2} \to C O_{2} (g); Δ H = - 94.5 K c a l

C (g r a p h i t e) + O_{2} \to C O_{2} (g); Δ H = - 94 K c a l

Δ H_{t}

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

Δ H = x k J

C (d i a m o n d) + O_{2} (g) \to C O_{2} (g)

Δ H = y k J

C (g r a p h i t e) + \frac{1}{2} O_{2} \to C O Δ H_{1} = - 110.5 k J / m o l

C O + \frac{1}{2} O_{2} \to C O_{2} Δ H = - 283.2 k J / m o l

k J / m o l

C (g r a p h i t e) + O_{2} \to C O_{2} Δ H = ?

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