The reaction between iron(II) oxide and carbon monoxide produces iron and carbon dioxide. How many moles of iron can be obtained when 1.50 mol FeO reacts with an excess of CO ? FeO+CO⟶Fe+CO2

1.5 moles of Fe can be obtained when 1.50 mol of FeO reacts with an excess

of CO

Moles of FeO reacted  = 1.50 mol

Moles of iron produced = ? mol

The chemical equation is given as

FeO + CO       →       Fe + CO₂

Comparisons of FeO and Fe show they are in the ratio 1 : 1

                          FeO          :           Fe

                            1.5           :           1.5

which translates to the number of moles being equal

Therefore, 1.5 moles of FeO 1.5 moles of Fe are produced.    

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1.5 moles of Fe produced.

Explanation:

Given data:

Moles of FeO react = 1.50 mol

Moles of iron produced = ?

Solution:

Chemical equation:

FeO + CO       →       Fe + CO₂

Now we will compare the moles of ironoxide with iron.

                           FeO          :           Fe

                              1             :             1

                             1.5           :           1.5

Thus from 1.5 moles of FeO 1.5 moles of Fe are produced.                                    

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

where's the diagram?