Determine the heat of transformation of C(diamond)→ C(graphite) from the following data.

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

$C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g) △ H = - 94.0 K c a l$

-0.5 K cal

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0.5 K cal

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188.5 K cal

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-188.5 K cal

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Solution

The correct option is A
-0.5 K cal

The equations given to us are as follows:

$C_{(d i a m o n d)} + O_{2} (g) \to C O_{2} (g) △ H = - 94.5 K c a l - - - - - - (i)$
$C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g) △ H = - 94.0 K c a l - - - - - - (i i)$
Now we subtract equation (ii) from (i) we get

$C_{(d i a m o n d)} \to C_{(g r a p h i t e)} △ H = - 0.5 K c a l$

Suggest Corrections

Similar questions

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

(i n k c a l)

C_{(d i o m o n d)} + O_{2} (g) \to C O_{2} (g) . . . (i) (Δ H = - 94.5 k c a l) C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g) . . . (i i) (Δ H = - 94.0 k c a l)

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

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

C_{(g r a p h i t e)} + O_{2} (g) \to C {C O}_{2} (g); (Δ H = - 94.0 k c a l)

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

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

C (d i a m o n d, s) \to C (g r a p h i t e, s)

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

C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g) △ H = - 94.0 K c a l

Δ H

C (g r a p h i t e) \to C (d i a m o n d)

C (g r a p h i t e) + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 393.5 k J

C (g r a p h i t e) + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 395.4 k J

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