So I have this question it reads

Consider the generic chemical reaction
How many moles of B are required to completely react with
2A + 3B ==> 3C
1. 6 mol of A
2. 2 mol of A
I won't put them all just guide me in the right direction please

I think I got it

6 mol A / 2 mol A x3 mol B = 9 mol B

You're right. This is the same kind of problem I worked in detail last night for you with the limiting reagent problem. The dimensional approach lets you see that the old units cancel and the new unit remains.

6 moles A x (3 moles B/2 mols A) = 9 moles B. Note how the mols A term cancels and that factor I have in parentheses converts moles A to moles B using the coefficients in the balanced equation.

To determine the number of moles of B required to completely react with a given amount of A, you can use the balanced chemical equation and calculate the stoichiometric ratio between A and B.

Let's start with option 1: "6 mol of A."

According to the chemical equation 2A + 3B ==> 3C, the stoichiometric ratio between A and B is 2:3. This means that for every 2 moles of A, you need 3 moles of B.

If you have 6 moles of A, you can set up a ratio based on the stoichiometry:

(3 mol B / 2 mol A) x 6 mol A = 9 mol B

So, with 6 moles of A, you would need 9 moles of B.

Now let's move to option 2: "2 mol of A."

Using the same stoichiometry, we can calculate the required moles of B:

(3 mol B / 2 mol A) x 2 mol A = 3 mol B

So, with 2 moles of A, you would need 3 moles of B.

Therefore, the answer to your question is:

1. For 6 moles of A, you need 9 moles of B.
2. For 2 moles of A, you need 3 moles of B.

Remember, to solve such problems, it's crucial to understand and apply the stoichiometry (mole ratio) given in the balanced chemical equation.

help????