Answer : The mass of
produced will be, 5.3 grams.
Explanation : Given,
Mass of
= 1.74 g
Mass of
= 11 g
Molar mass of
= 58 g/mole
Molar mass of
= 32 g/mole
Molar mass of
= 44 g/mole
First we have to calculate the moles of
and
.


Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,

From the balanced reaction we conclude that
As, 2 moles of
react with 13 mole of 
So, 0.03 moles of
react with
moles of 
From this we conclude that,
is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of
.
As, 2 moles of
react to give 8 moles of 
So, 0.03 moles of
react to give
moles of 
Now we have to calculate the mass of
.


Therefore, the mass of
produced will be, 5.3 grams.