Question

Balance the following equation:

NHa(g) + F2(g) - NaF4(g) + HF(g)
a. How many moles of each reactant are needed to produce 4.00 moles of HF?
b. How many grams of F2 are required to react with 1.50 moles of NH;?
c. How many grams of N2F4 can be produced when 3.40 grams of NHs reacts?

Answer 1

Answer:NH3: 4.00 moles

F2: 4.00 moles

Explanation:The balanced equation for the given chemical reaction is:

NH3(g) + F2(g) → NF3(g) + HF(g)

According to the balanced equation, 1 mole of NH3 reacts with 1 mole of F2 to produce 1 mole of NF3 and 1 mole of HF.

To produce 4.00 moles of HF, we need to determine how many moles of NH3 and F2 are required. Since the mole ratio between NH3 and HF is 1:1, we would need 4.00 moles of NH3. Similarly, since the mole ratio between F2 and HF is also 1:1, we would need 4.00 moles of F2 as well.

So, the answer is:

NH3: 4.00 moles

F2: 4.00 moles