Question

Diamond and graphite, burn to give out:
A) Carbon monoxide
B) Carbon dioxide
C) Carbon
D) Oxygen

Answer 1

Hint:Carbon and graphite both are the allotropes of carbon. Thus, on consuming in air at high temperature carbon consolidates with environmental oxygen to give just $C{O}_2$ and no building is abandoned. Diamond and graphite are allotropes of carbon and they give a compound of carbon during burning.

Complete step by step answer:
As crystalline carbon, diamonds have precisely the same structure as graphite (however they have distinctive subatomic structures). On the off chance that the unequivocally warmed within the sight of oxygen, carbon will respond with the oxygen (consume) to shape carbon dioxide gas ($C{O}_2$).
Different mixes containing carbon for example plant material as substance will break down immediately when warmed firmly. At typical temperature and within the site of dampness and microscopic organisms, they will disintegrate gradually into different gases including methane ($C{H}_4$) and carbon dioxide ($C{O}_2$).
$$\begin{gathered} C(graphite)+O_2\to C{O}_2 \\ C(diamond)+O_2\to C{O}_2 \end{gathered}$$
Allotropy= the phenomenon of existence of an element in two or more forms which have different physical properties but identical chemical properties is called allotropy and the different forms are called allotropic forms or simply allotropic forms. These are
Diamond
Graphite
Fullerenes
Diamond= crystals found in nature are generally octahedral. In the structure of diamond each carbon is linked to the four other carbon atoms forming a regular tetrahedral arrangement and this network of carbon atoms extends in three dimensions and is very rigid. Elements in which atoms are bonded covalently e sound in solid state.
Graphite= graphite is a great choice black substance. It occurs in nature. Each carbon is bonded to you only three neighbouring carbon atoms in the same plane forming layers of hexagonal networks separated by comparatively large distance. The different layers are held together by weak forces called Wonderwall forces. The layer can therefore easily slide over one another. This makes purified lubricating, soft and greasy to touch.
Reference of carbon with $$O_2$$:
Carbon is graphite consumed to frame vaporous carbon dioxide. Graphite is a type of carbon and furthermore consumes in air when warmed to $${600}^{\circ }C-{800}^{\circ }C$$a costly method to make carbon dioxide.
$C_g+O_2\to C{O}_2$
($\mathrm{\Delta }H=-393.5KJ$)
 At the point when the air of oxygen gracefully is limited fragmented ignition two carbon monoxide happens.
$C_{\left(O\right)}+O_2\to C{O}_2$
($\mathrm{\Delta }H=-395.4KJ$)
This response is significant. In industry air is blown through hot coke. The subsequent gas is called maker gas and is a combination of carbon monoxide $$\left(25\mathrm{\%}\right)$$, carbon dioxide $$\left(4\mathrm{\%}\right)$$, nitrogen $$\left(70\mathrm{\%}\right)$$, and hints of hydrogen Methane and oxygen.
 Hence, option B is correct.

Note:
A diamond is the hardest natural substance on earth but if it is placed in an oven and the temperature is raised to about $${763}^{\circ }C$$ it will simply vanish without even remaining only a little carbon dioxide will have been released.
 Diamond has a three-dimensional network structure graphite has it two-dimensional sheet like structure consisting of a number of benzene rings fused together