when carbon combines with oxygen to form carbon dioxide, ratio is 3:8. when carbon combines with oxygen to form carbon monoxide, ratio is 1:2. is this right? if it is, could u please explain? if it isn't please correct it and explain.
Answers
Answer:
Chemical reactions are described by chemical equations.
Example: The reaction between hydrogen and oxygen to form water is represented by the following equation.
2 H2 + O2-----> 2 H2O
It is often useful to indicate whether the reactants or products are solids, liquids, or gases by writing an s, l, or g in parentheses after the symbol for the reactants or products, as shown in the following equations.
2 H2(g) + O2(g) -----> 2 H2O(g)
2 Al(s) + Fe2O3(s) -----> Al2O3(s) + 2 Fe(l)
Because so many reactions occur when solutions of two substances dissolved in water are mixed, a special symbol, aq, is used to describe these aqueous solutions.
The process in which a sample dissolves in water will be indicated by equations such as the following.
H2O
C12H22O11(s) C12H22O11(aq)
A chemical equation is a statement of what can happen, not necessarily what will happen. The following equation, for example, does not guarantee that hydrogen will react with oxygen to form water.
2 H2(g) + O2(g) -----> 2 H2O(g)
It is possible to fill a balloon with a mixture of hydrogen and oxygen and find that no reaction occurs until you touch the balloon with a flame. The balanced equation for this reaction describes the relationship between the amounts of hydrogen and oxygen consumed and the water formed if or when this reaction is initiated.
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Equations at the Atomic and Macroscopic Scale
Chemical equations can be used to represent what happens on either the atomic or macroscopic scale.
2 H2(g) + O2(g) -----> 2 H2O(g)
This equation can be read in either of the following ways.
If, or when, hydrogen reacts with oxygen, two molecules of hydrogen and one molecule of oxygen are consumed for every two molecules of water produced.
If, or when, hydrogen reacts with oxygen, two moles of hydrogen and one mole of oxygen are consumed for every two moles of water produced.
Chemical equations must be balanced -- they must have the same number of atoms of each element on both sides of the equation. As a result, the mass of the reactants must be equal to the mass of the products of the reaction. On the atomic scale, the following equation is balanced because the total mass of the reactants is equal to the mass of the products.
2 H2(g) + O2(g) -----> 2 H2O(g)
2 x 2 amu + 32 amu 2 x 18 amu
bracket bracket
36 amu 36 amu
On the macroscopic scale, it is balanced because the mass of two moles of hydrogen and one mole of oxygen is equal to the mass of two moles of water.
2 H2(g) + O2(g) -----> 2 H2O(g)
2 x 2 g + 32 g 2 x 18 g
bracket bracket
36 g 36 g
Explanation: