Question

HELP!
Suppose 4.0 grams of H2 were used? How many grams of water would be produced?

Answer 1

Answer:

36g

             

Explanation:

Given parameters:

Mass of H₂  = 4g

Unknown:

Mass of water produced  = ?

Solution:

The reactants in this experiment are hydrogen and oxygen gas. The product formed will be water, H₂O.

 Now write the reaction equation first;

                   2H₂  + O₂  →  2H₂O

Find the number of moles of Hydrogen gas;

         Number of moles  = $\frac{mass}{molar mass}$  

  Molar mass of H₂  = 2(1) = 2g/mol

        Number of moles  = $\frac{4}{2}$   = 2moles

From the balanced reaction equation;

             2 moles of H₂ will produce 2 moles of H₂O

So, mass of H₂O produced;

        Mass of H₂O = number of moles x molar mass

   Molar mass of H₂O  = 2(1) + 16  = 18g/mol

    Mass of H₂O  = 2 x 18 = 36g

             

Answer 2

We can see from the calculations that the use of 4g of hydrogen produces 36 g of water.

We know that water is produced from the equation;

2H2(g) + O2(g) ----> 2H2O(g)

Number of moles of hydrogen = 4 g/2 g/mol = 2 moles of hydrogen

From the reaction equation, we can see that 2 moles of hydrogen yields 2 moles of water.

Hence, If we use 4g  of hydrogen, we end up with 2 moles of water.

Mass of water = 2 * 18 g/mol = 36 g

Learn more about stoichiometry: https://brainly.com/question/1301963