When 3.0 g of carbon is burnt in 8.0 g of oxygen, 11.0 g of carbon dioxide is produced. what is the mass of carbon dioxide will be formed when 3.0 g of carbon is burnt in 50.0 g of oxygen? Which law of chemical combination will govern the answer?

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When 3.0 g of carbon is burnt in 8.0 g of oxygen, 11.0 g of carbon dioxide is produced. what is the mass of carbon dioxide will be formed when 3.0 g of carbon is burnt in 50.0 g of oxygen? Which law of chemical combination will govern the answer?

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Answer 1 · 2016-11-23T09:07:55

A mass of $11.0 \cdot g$ $11.0*g$ of carbon dioxide will again be produced.

Explanation:

When a $3.0 \cdot g$ $3.0*g$ mass of carbon is burnt in an $8.0 \cdot g$ $8.0*g$ mass of dioxygen, the carbon and the oxygen are stoichiometrically equivalent. Of course, the combustion reaction proceeds according to the following reaction:

$C (s) + O_{2} (g) \to C O_{2} (g)$ $C(s) + O_2(g) rarr CO_2(g)$

When a $3.0 \cdot g$ $3.0*g$ mass of carbon is burnt in an $50.0 \cdot g$ $50.0*g$ mass of dioxygen, the oxygen is present in stoichiometric excess. The $42.0 \cdot g$ $42.0*g$ excess of dioxygen is along for the ride.

The law of conservation of mass, $garbage in equals garbage out$ $"garbage in equals garbage out"$ , applies for both examples.

Most of the time, in coal-fired generators, and certainly in the internal combustion engine, carbon oxidation is incomplete, and $C O$ $CO$ gas and particulate carbon as soot, are products with $C O_{2}$ $CO_2$ .

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When 3.0 g of carbon is burnt in 8.0 g of oxygen, 11.0 g of carbon dioxide is produced. what is the mass of carbon dioxide will be formed when 3.0 g of carbon is burnt in 50.0 g of oxygen? Which law of chemical combination will govern the answer?

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Explanation:

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