# Limiting and Excess Reactants in Redox

## Homework Statement

Suppose 1.00g of Mn Reacts with an excess of 6.00M HCl, how many grams of H2 gas is produced?
What volume hydrogen gas is produced by this reaction?

## Homework Equations

density of hydrogen gas is 0.08988g/L
conditions: 0 degrees celsius, 1 atm pressure

## The Attempt at a Solution

First I wrote the reaction out

2Mn +6HCl -> 2MnCl3 +3H2

Then this is where I ran into some confusion. Does the 6.00M solution have any effect on the amount of hydrogen produced? I assumed it did not and then went on to find the moles of Mn ( 0.0182 mol) and used the molar ratio of 2:3 to find out the moles of hydrogen gas (0.0273 mol).

I then determined the grams of hydrogen gas and then used a comparison ratio between it and the density of hydrogen gas to find the volume which I determined to be 0.612L.

I just require some verification, from what I remember the limiting reactant is what determines the amount of moles produced

You are OK being wrong 