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

1.326 grams of NH3 are required to produce 4.65 g of HF.

Step-by-step explanation:

Balanced chemical reaction is written first to know the number of moles taking part in original reaction.

NH3 +3 F2 ⇒3 HF  +  NF3

Given:

mass of HF = 4.65

First the number of moles of HF in 4.65 grams is calculated by using the formula:

number of moles (n) =

atomic mass of HF = 20 grams/mole

putting the values in the above equation number of moles can be found.

n =

  = 0.235 moles of HF are given.

From the equation it can be said that:

1 mole of NH3 reacts to form 3 moles of HF

so, x moles of NH3 would react to form 0.235 moles of HF

=

3x = 0.235

x =

x = 0.078 moles of NH3 is required.

The moles are converted to mass by applying the formula:

mass = atomic mass X number of moles (atomic mass of NH3 = 17 grams/mole)

        putting the values in the formula

mass = 17 X 0.078

mass = 1.326 grams

There are a few ways to find out the correct answer. One of them is to divide 2.40 by 6 to get a price of one cake and then multiply it by 10:

2.40 ÷ 6 = 0.40

0.40 * 10 = 4.00

Ten cakes would cost 4 pounds.