Calculate the number of grams of fe2o3 needed to react with 19.0 g c.

The mass of iron (III) oxide needed to react is 67.4 g

Explanation:

To calculate the number of moles, we use the equation:

     .....(1)

Given mass of carbon = 19.0 g

Molar mass of carbon = 12 g/mol

Putting values in equation 1, we get:

The chemical equation for the reaction of iron (III) oxide and carbon follows:

By Stoichiometry of the reaction:

3 moles of carbon reacts with 2 moles of iron (III) oxide

So, 1.58 moles of carbon will react with = of iron (III) oxide

Now, calculating the mass of iron (III) oxide by using equation 1, we get:

Molar mass of iron (III) oxide = 159.70 g/mol

Moles of iron (III) oxide = 0.422 moles

Putting values in equation 1, we get:

Hence, the mass of iron (III) oxide needed to react is 67.4 g

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

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