In a certain reaction, 300.23 grams of solid aluminum sulfide combine with unlimited aqueous silver nitrate. How many moles of aluminum sulfide react? How many moles of each product will be produced?

First of all, is the reaction a double replacement or not? I have so much trouble with chem! Please help!

The reaction is:

Al2S3 + 6AgNO3(aq) --> 3Ag2S(s) + 2Al(NO3)3(aq)
Find the formula mass (molar mass) of Al2S3.
Divide 300.23 g by the formula mass to get moles of Al2S3.

Moles of Ag2S = (__moles Al2S3)(3)
Moles of Al(NO3)3 = (__moles Al2S3)(2)

double replacement.

YOu always start with the balanced chem reaction:

Al2S3 + 6AgNO3 >>3Ag2S+2Al(NO3)3
and the silver sulfide precipates out of solution.

So for each mole of aluminum sulfide, you get three moles of silver sulfide, and two moles of aluminum nitrate.

So how many moles of aluminum sulfide are in 300.23 grams? You get three times that number of moles of Ag2S, and twice that number of moles of Aluminum nitrate.

To determine the type of reaction, we need to write the balanced chemical equation.

The balanced chemical equation for the reaction between aluminum sulfide (Al2S3) and silver nitrate (AgNO3) is:

Al2S3 + 6AgNO3 → 2Al(NO3)3 + 3Ag2S

Looking at this equation, we can see that the reactants (aluminum sulfide and silver nitrate) are swapping partners to form new products (aluminum nitrate and silver sulfide). This is known as a double replacement reaction.

Now, let's move on to calculating the number of moles involved in the reaction.

Step 1: Convert the mass of aluminum sulfide to moles.
To do this, we need to know the molar mass of aluminum sulfide (Al2S3). By using the atomic masses from the periodic table, we calculate:

2(Al) + 3(S) = (2)(26.98 g/mol) + (3)(32.07 g/mol) = 37.96 g/mol + 96.21 g/mol = 134.17 g/mol

Now, we can calculate the number of moles of aluminum sulfide:
Number of moles = mass / molar mass
Number of moles = 300.23 g / 134.17 g/mol = 2.2406... moles (rounded to four decimal places)

Therefore, 2.2406 moles of aluminum sulfide react.

Step 2: Calculate the number of moles of each product.
By looking at the balanced chemical equation, we can see that for every 2 moles of aluminum sulfide, 2 moles of aluminum nitrate (Al(NO3)3) and 3 moles of silver sulfide (Ag2S) are produced.

So, the number of moles of Al(NO3)3 produced is:
Number of moles of Al(NO3)3 = 2.2406 moles × (2 moles of Al(NO3)3 / 2 moles of Al2S3) = 2.2406 moles

The number of moles of Ag2S produced is:
Number of moles of Ag2S = 2.2406 moles × (3 moles of Ag2S / 2 moles of Al2S3) = 3.3609 moles

Therefore, 2.2406 moles of aluminum nitrate and 3.3609 moles of silver sulfide will be produced.