# If 5.00g of MnO2 reacts w/ 25.0mL of 6M HCL calculate the mass of Cl2 produced? I figured out MnO2 but stuck with HCl. I did 25mL HCl x(0.001L/1mL)x (6mol HCl/1 L) but I don't know where I should go now?

##### 1 Answer

This reaction will produce

Start with the balanced chemical equation, that is *a must* for any stoichiometry problem.

Now look at the mole ratios you have between **1 mole** of *needs* **4 moles** of *in order to produce* **1 mole** of

SInce you can calculate how many moles of both

Use the molarity of the

However, according to the mole ratio, you would have needed

This means that *actually reacts*

This will be equal to the number of

You can adjust this to the number of sig figs you actually have, since I think 6 M was actually 6.0, or 6.00 M.

**SIDE NOTE** The net ionic equation for this reaction is