1. Given the reaction:

2 A1 + 3 H2SO4 -- A12(SO4)3 + 3 H2
If an excess of sulfuric acid is combind with 10.0g of aluminum, and 0.150g of hydrogen is obtained, what is the percentage yield of the hydrogen? EXPLAIN ALL STEPS THIS NEEDS TO BE DONE BY TONIGHT SO I HOPE I CAN GET HELP!

Question

1. Given the reaction:

2 A1 + 3 H2SO4 --> A12(SO4)3 + 3 H2
If an excess of sulfuric acid is combind with 10.0g of aluminum, and 0.150g of hydrogen is obtained, what is the percentage yield of the hydrogen? EXPLAIN ALL STEPS THIS NEEDS TO BE DONE BY TONIGHT SO I HOPE I CAN GET HELP!

anonymous · Answer

If u help me ill help you..

anonymous · Answer

do u know the answer to my problem?

anonymous · Answer

yes help me first I promise ill help u..

anonymous · Answer

This is one possible reaction, and it may or may not be the energetically favored one. I start by just writing it out, without any stoichiometric coefficients: 

Al + H2SO4 ===> Al2(SO4)3 + H2 

Next, I balance it element by element, starting with aluminum. 

2Al + H2SO4 ===> Al2(SO4)3 + H2 

There are two Al's on each side, so that's balanced. Next I take care of sulfate ions: 

2Al + 3H2SO4 ===> Al2(SO4)3 + H2 

There are 3 SO4's on each side. Since the only source of oxygen is sulfate, this shortcut worked, and all that's left is the hydrogen on the right side. I balance it as follows: 

2Al + 3H2SO4 ===> Al2(SO4)3 + 3H2 

This reaction was pretty simple, but if it was more complicated, you could use matrix methods. For any hypothetical reaction, if you can write a system of linearly independent equations, you can find a set of stoichiometric coefficients. 

To do this, set up a matrix, with one row for each element, and one column for each species. For each entry in the matrix, put in the number of atoms of that element in that species. Make this number negative if it is in a reactant, and positive if it is in a product. Then, add a column of all zeros on the right side. Finally, add a row to the bottom that defines your basis (like one mole of aluminum). 

Let's say I'd assumed the other product was water, not hydrogen. The reaction would be: 

Al + H2SO4 ===> Al2(SO4)3 + H2O

anonymous · Answer

Can you help me with like 6 more please?

anonymous · Answer

I Can try.

anonymous · Answer

2. Chlorine gas can be produced from the reaction of manganese(IV) oxide with hydrochloric acid as shown in the following equation:

 MnO2 + 4 HC1 --> MnC12 + 2 H2O + C12

How many grams of chlorine can be produced from 76.0 g of MnO2 (assume sufficient HC1)?

anonymous · Answer

6.22 grams

anonymous · Answer

can u explain?