How many grams of NH3 are required to produce 4.65 g of HF

1.32g

Explanation:

Given parameters:

Mass of HF   = 4.65g

Unknown:

Mass of NH₃ = ?

Solution:

We need to know the reaction equation first of all. The reaction that will produce HF involves;

                 2NH₃    +    5F₂    →    N₂F₄   + 6HF

Now that we know the reaction equation;

Find the number of moles of the HF;

        Number of moles  =

         Molar mass of HF  = 1 + 19 = 20g/mol

        Number of moles  =   = 0.23mole

From the balanced reaction equation;

        6 moles of HF is produced from 2 moles of NH₃  

        0.23 moles of HF will be produced from      = 0.08moles

Now we find the mass of NH₃

          Mass of NH₃ = number of moles x molar mass

                   Molar mass of NH₃  = 14 + 3(1) = 17g/mol

         Mass of NH₃   = 0.08 x 17  = 1.32g

explanation:

two years ago, when picking flowers in the mountains back of yosemite valley, i found a book. it was blotted and storm-beaten; all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however; many of the inner pages were well preserved. and although all were more or less stained and torn, whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today; its granite pages have been torn and blurred by the same storms that wasted the castaway book.

two years ago, when picking flowers in the mountains back of yosemite valley; i found a book. it was blotted and storm-beaten, all of its outer pages were mealy and crumbly. the paper seemed to dissolve like the snow beneath which it had been buried, however, many of the inner pages were well preserved. and although all were more or less stained and torn; whole chapters were easily readable. this is the condition of the great open book of yosemite glaciers today, its granite pages have been torn and blurred by the same storms that wasted the castaway book.