How many grams of silver nitrate are required to produce 4.2 moles of silver nitrate

Question

2AgNO3 + H2S -> Ag₂S + 2HNO₃

Answer 1

2AgNO₃ + H₂S -> Ag₂S + 2HNO₃

Karim,

I am assuming that the last part of the question must be silver sulfide. That is the only product conatining silver.

In any balanced chemical equations, the coefficients (number infront of each reactant and product) give you the mole-to-mole ratios.

2 mol AgNO3 produces 1 mole of Ag2S.

We can get two possible ratios:

(i) (2mol AgNO3/1 mol Ag2S)

(ii) (1mol Ag2S/2 molAgNO3)

If we want to find how many grams of AgNO3 required, we will use the first ratio.

4.2 mol Ag2S (2 mol AgNO3/1 mol Ag2S) = 8.4 mol AgNO3 is required. Note: Look at how the units cancel out.

Then you can convert 8.4 mol AgNO3 into g of AgNO3 using the mola mass of AgNO3 (169.87 g/mol)

8.4 mol AgNO3 (169.78 gAgNO3/1mol AgNO3) = 1426.1 g AgNO3 is required.

T. Degefa