Consider the following reaction. how many moles of oxygen are required to produce 2.33 moles of water? assume that there is excess c3h7sh present.

3.5 moles of oxygen are required to produce 2.33 moles of water

Stoichiometry in Chemistry learn about chemicals mainly emphasizes quantitative, such as the calculation of volume, mass, number, which is related to numbers, molecules, elements, etc.

A reaction coefficient is a number in the chemical formula of a substance involved in the reaction equation. The reaction coefficient is useful for equalizing reagents and products.

In the reaction there are also manifestations of reagent substances namely gas (g), liquid (liquid / l), solid (solid / s) and solution (aqueous / aq).

The concentration of a substance can be expressed in several quantities such as moles, percent (%) weight/volume,), molarity, molality, parts per million (ppm) or mole fraction. The concentration shows the amount of solute in a unit of the amount of solvent.

The mole itself is the number of particles contained in a substance amounting to 6.02.10²³

Mole can also be sought if the amount of substance mass and its molar mass is known

Reaction that happens :

C₃H₇SH (l) + 6 O₂ (g) ⇒3 CO₂ (g) + SO₂ (g) + 4 H₂O (g)

And because C₃H₇SH (l) ) is excess reactant, O₂ functions as a limiting reagent, so the determination of H₂O mole based on O₂ mole

From the coefficient of the equation above, it shows that the ratio of mol O₂: mol H₂O = 6: 4

So to produce 2.33 moles of H₂O, O₂ is needed as much as:

mole O₂ = 6/4 x 2.33

mole O₂ = 3,495 = 3.5 mole

The mass of one mole of raindrops

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moles of NaOH

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moles of water you can produce

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Keywords: mole, excess, limiting reactants, H₂O

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