Two reactions are given below- Cgraphite - O2g- CO2g- - H - -393-7 kJ Cdiamond- Cgraphite- - H - -2-1 kJWhat quantity of diamond will give 800 kJ of heat on burning-

The correct option is D 24.25 g C_diamond + O_2(g)→ CO_2 . Δ H= 393.7 + ( 2.1) = 395.8 kJ/mol 12 g diamond gives 395.8 kJ of heat. 80 ...

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Introduction

Two reactions...

Question

Two reactions are given below:

$C_{(g r a p h i t e)} + O_{2 (g)} \to C O_{2 (g)}; Δ H = - 393.7 k J$
$C_{(d i a m o n d)} \to C_{(g r a p h i t e)}; Δ H = - 2.1 k J$

What quantity of diamond will give 800 kJ of heat on burning?

24.25 g

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15.24 g

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2 g

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12.12 g

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Solution

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Similar questions

C_{D i a m o n d} + O_{2} \to C O_{2} (g); Δ H = - 94.3 k c a l

C_{G r a p h i t e} + O_{2} \to C O_{2} (g); Δ H = - 97.6 k c a l

C_{d i a m o n d} \to C_{g r a p h i t e}

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

$Δ H = - 393.5 k . J$

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

$Δ H = - 395.4 k . J$

Reason(R): graphite is more stable than diamond, so heat of combustion is less.

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

5000 k J

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) + O_{2} (g) ⟶ C O_{2} (g); Δ H = - 393.7 k J

C (d i a m o n d) ⟶ C (g r a p h i t e); Δ H = - 2.1 k J

Δ H

C O_{2}

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