How many moles of methane are produced when 48.1 moles of carbon dioxide react with excess hydrogen gas?

The number of moles of methane, CH₄ produced is 48.1 moles

We'll begin by writing the balanced equation for the reaction. This is given below:

From the balanced equation above,

1 mole of CO₂ reacted to produce 1 mole of CH₄.

Finally, we shall determine the number of mole of CH₄ produced by the reaction of 48.1 moles of CO₂. This can be obtained as follow:

From the balanced equation above,

1 mole of CO₂ reacted to produce 1 mole of CH₄.

Therefore,

48.1 moles of CO₂ will also react to produce 48.1 moles of CH₄.

Thus, 48.1 moles of CH₄ were obtained from the reaction.

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48.1 moles methane are produced when 48.1 moles of carbon dioxide react with excess hydrogen

Stochiometry in Chemistry learns about chemical reactions mainly emphasizing quantitative, such as calculation of volume, mass, number, which is related to the number of ions, molecules, elements, etc.

In chemical calculations, the reaction can be determined, the number of substances that can be expressed in units of mass, volume, mole, or determine a chemical formula, for example, the substance level or molecular formula of the hydrate.

The reaction equation is the chemical formula of reagents and product substances

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

Reaction that happens between carbon dioxide with the hydrogen

CO₂ + 4H₂ ---> CH₄ + 2H₂O

And because hydrogen is excess reactant, CO₂ functions as a limiting reagent, so the determination of CH₄ mole based on CO₂ mole

From the coefficient of the equation above, it shows that the ratio of mol CO₂: mol CH₄ = 1 : 1

So from 48.1 moles of CO₂ will produce CH₄ of 48.1 moles

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Keywords: mole, excess, limiting reactants, H₂O

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

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c (diamond),

sio2 (quartz)