How many grams of #H_2O# will be produced if 750 grams of #Fe# are produced in the equation #Fe_3O_4 + H_2 -> Fe + H_2O#?

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Answer 1 · 2017-09-10T12:50:56

Approx.....#300*g# water are evolved......

We need (i) a stoichiometric equation......

#Fe_3O_4 + 4H_2 rarr 3Fe+4H_2O#

And thus for each mole of iron produced, #4/3# mol of water are produced consequently......

And (ii) we work out the equivalent quantity of metal.....

#"Moles of iron"-=(750*g)/(55.8*g*mol^-1)=13.44*mol#

And so we take the product.....

#13.44*molxx4/3xx18.011*g*mol^-1=323*g# with respect to water.....