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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: renilee on October 05, 2011, 08:58:31 PM

Title: What mass of aluminum sulfate would be produced with this formula?
Post by: renilee on October 05, 2011, 08:58:31 PM

I would love some help with this! I tried several different ways but I just don't understand how to find the answer to this, unfortunately. It's stressing me out quite a bit...

Given: 2Al(s) + H2SO4(aq) → 3H2(g)+Al2(SO4)3(s)  (already balanced)

If you mixed 0.809 g of Al with 1.40 g of H2SO4, what mass of aluminum sulfate would be produced?


I also have another question about joules:

Given: 2H2 (g) + O2 (g) → 2H2O(g) + 562 joules

What mass of fuel (hydrogen) has to be burned to produce 2.99 x 106 joules of heat?
 ___ grams

At STP, what volume of oxygen would be consumed in the production of 2.99 x 106 joules of heat?
____ L

Thanks so much! ><

Title: Re: What mass of aluminum sulfate would be produced with this formula?
Post by: Borek on October 06, 2011, 02:45:10 AM

You have to show your attempts at solving the question to receive help. This is a forum policy.

http://www.chembuddy.com/?left=balancing-stoichiometry&right=limiting-reagents