According to this chemical reaction, which is the number of grams of fe produced from 14 moles of h2? fe3o4 + 4 h2 → 3 fe + 4 h2o

From the equation of the reaction,  the mass of Fe produced from 14 moles of H₂ is 588 g.

The equation of the reaction is given as follows:

From the equation of the reaction, 4 moles of H₂ produces 3 moles of Fe.

14 moles of H₂ will produce 14 * 3/4 moles of Fe = 10.5 moles of Fe.

Mass of 10.5 moles of Fe = 56 * 10.5

Mass of 10.5 moles of Fe = 588 g

Therefore, the mass of Fe produced from 14 moles of H₂ is 588 g.

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Explanation:

We know we will need a balanced equation with masses, moles, and molar masses, so let’s gather all the information in one place.

M_r:                            55.85  

            Fe₃O₄ + 4H₂ → 3Fe + 4H₂O

n/mol:                  14

1. Use the molar ratio of Fe:H₂ to calculate the moles of Fe.

2. Use the molar mass of Fe to calculate the mass of Fe

the only liquid elements at standard temperature and pressure are bromine (br) and mercury (hg). although, elements caesium (cs), rubidium (rb), francium (fr) and gallium (ga) become liquid at or just above room temperature.

explanation:

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