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quasarJose

Explanation:

The reaction expression is given as:

           2H₂  +   O₂    →    2H₂O

The limiting reactant is the reactant in short short supply in the given reaction.

To find the limiting reactant we use the number of moles.

    Mass of H₂  = 5g

    Mass of O₂   = 10g

  Number of moles  = [tex]\frac{mass}{molar mass}[/tex]  

       Molar mass of H₂   = 2(1) = 2g/mol

       Molar mass of O₂  = 2(16)  = 32g/mol

Number of moles  H₂ = [tex]\frac{2}{5}[/tex]   = 0.4mole

Number of moles O₂ = [tex]\frac{10}{32}[/tex]   = 0.3mole

   From the balanced reaction equation:

           2 mole of H₂ reacts with 1 mole of O₂

          0.4 mole of H₂ reacts with  0.2 mole of O₂

But we are given 0.3 moles of O₂, so the limiting reactant is H₂ because oxygen gas is in excess

The limiting reactant when 5.00g of H₂ and 10.00g of O₂ react is Oxygen (O₂)

Stoichiometry

From the question,

We are to determine the limiting reactant

First, we will write the balanced chemical equation for the reaction

The balanced chemical equation for the reaction is

2H₂ + O₂ → 2H₂O

This means 2 moles of H₂ reacts with 1 mole of O₂ to produce 2 moles of H₂O

Now, we will determine the number of moles of each reactant present

  • For H₂

Mass = 5.00 g

Molar mass = 2.0 g/mol

Using the formula,

[tex]Number\ of \ moles = \frac{Mass}{Molar\ mass}[/tex]

Number of moles of H₂ = [tex]\frac{5.00}{2.0}[/tex]

Number of moles of H₂ = 2.50 moles

  • For O₂

Mass = 10.00 g

Molar mass = 32.0 g/mol

Then,

Number of moles of O₂ = [tex]\frac{10.00}{32.0}[/tex]

Number of moles of O₂ = 0.3125 mole

Now,
Since 2 moles of H₂ reacts with 1 mole of O₂

Then,

0.625 moles of H₂ reacts with 0.3125 mole of O₂

This means part of the H₂ reacts with all of the O₂. Since all the O₂ reacted, then O₂ is the limiting reactant.

Hence, the limiting reactant when 5.00g of H₂ and 10.00g of O₂ react is Oxygen (O₂).

Learn more on Stoichiometry here: https://brainly.com/question/17199947

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