Question

what is the mass of a product if the reactants masses are 11.26g hydrogen and 88.26g oxygen?

Answer 1

The mass of the product (water) if the reactants masses are 11.26g hydrogen and 88.26g oxygen is 99.37g

From the question,

We are to determine the mass of the product formed from reacting 11.26g hydrogen and 88.26g oxygen.

The product of the reaction is water.

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

The balanced chemical equation for the reaction between hydrogen and oxygen is

2H₂ + O₂ → 2H₂O

This means,

2 moles of Hydrogen reacts with 1 mole of Oxygen to produce 2 moles of water

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

For Hydrogen

Mass of hydrogen present = 11.26g

Molar mass of hydrogen = 2.016 g/mol

Using the formula

$Number\ of\ moles = \frac{Mass}{Molar\ mass}$

∴ Number of moles of hydrogen present = $\frac{11.26}{2.016}$

Number of moles of hydrogen present = 5.5853 moles

For Oxygen

Mass of oxygen present = 88.26g

Molar mass of oxygen = 32 g/mol

∴ Number of moles of oxygen present = $\frac{88.26}{32}$

∴ Number of moles of oxygen present = 2.7581 moles

Now,

Since

2 moles of Hydrogen reacts with 1 mole of Oxygen to produce 2 moles of water

Then,

5.5162 moles of Hydrogen will react with 2.7581 moles of Oxygen to produce 5.5162 moles of water

∴  Number of moles of the product (water) produced = 5.5162 moles

Now, for the mass of product

Using the formula

Mass =  Number of moles × Molar mass

Molar mass of water = 18.015 g/mol

∴ Mass of water produced =  5.5162 × 18.015

Mass of water produced = 99.374343g

Mass of water produced ≅ 99.37g

Hence, the mass of the product (water) if the reactants masses are 11.26g hydrogen and 88.26g oxygen is 99.37g

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