Phosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decoxide and water, as described by the following unbalanced equation. ph3(g) + o2(g) → p4o10(s) + h2o(g) calculate the mass of p4o10(s) formed when 225 g

The amount of formed is 469.8 grams.

Explanation:

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

    ......(1)

Given mass of phosphine = 225 g

Molar mass of phosphine = 34 g/mol

Putting values in equation 1, we get:

The given chemical reaction follows:

Assuming that oxygen gas is present in excess, it is considered as an excess reagent.

Phosphine is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

4 moles of phosphine produces 1 mole of

So, 6.62 moles of phosphine will produce = of

Now, calculating the mass of by using equation 1:

Molar mass of = 283.9 g/mol

Moles of = 1.655 moles

Putting values in equation 1, we get:

Hence, the amount of formed is 469.8 grams.