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C(("graphite")) + O(2(g)) to CO(2(g)) - ...

`C_(("graphite")) + O_(2(g)) to CO_(2(g)) - 94.0` kcal

A

endothermic

B

exothermic

C

decomposition

D

dissociation

Text Solution

Verified by Experts

The correct Answer is:
B
exothermic
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N_(2(g)) + O_(2(g)) to 2N_((g)) - 42.0 kcal

Calculate the standard enthalpy of the reaction, 2C_(("graphite")) + 3 H_(2(g)) to C_(2) H_(6(g)) Delta H^(@) = ? from the following Delta H^(@) values: (a) C_(2) H_(6(g)) + (7)/(2) O_(2(g)) to 2CO_(2(g)) + 3H_(2) O_((1)) Delta H^(@) = - 1560 kJ (b) H_(2(g)) + (1)/(2) O_(2(g)) to H_(2) O_((1)) Delta H^(@) = - 285.8 kJ (c ) C_(("graphite")) + O_(2(g)) to CO_(2(g)) Delta H^(@) = - 393.5 kJ

For the following reaction, C_("diamond")+O_(2)toCO_(2)(g), DeltaH=-94.3" "kcal C_("graphite")+O_(2)toCO_(2)(g), DeltaH=-97.6" "kcal the heat require to change 1 g of C_("diamond")toC_("graphite") is:

C_("graphite")+O_(2)(g)rarrCO_(2)(g) deltaH=-94.05Kcalmol^(-1) C_("diamond")+O_(2)(g),DeltaH=-94.50Kcalmol^(-1) Therefore,

For the following reaction, {:(C("diamond")+O_(2)to CO_(2)(g),, DeltaH=-97.6kcal),(C("graphite")+O_(2)to CO_(2)(g),,DeltaH=-94.3kcal):} The heat change for the conversion of 1 g of C (diamond) to C(graphite) is: