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April 18, 2014

April 18, 2014

Posted by **John** on Thursday, January 5, 2012 at 2:41am.

I'd appreciate any help I can get from anyone here to help me solve this problem:

Hydrogen and sulfur chemically combine to form the gas hydrogen sulfide, according to the reaction: H2 (g) + S(s) → H2S(g). How many liters of hydrogen are required to form 7.4 L of hydrogen sulfide (at STP: 273 K, 101.3 kPa)?

I know that it involves stoichiometry, and the Ideal Gas Law, but am kind of confused on how to start it.

Thank you in advance!

- chemistry -
**drwls**, Thursday, January 5, 2012 at 4:36amYour equation is balanced as written.

It tells you that the number of H2S moles formed equals the number of H2 moles reacted. Since you have defined the temperature and pressure of reactants and product to be the same, the number of liters of H2 and H2S are also the same.

The answer is 7.4 Liters. You do not have to use the gas law.

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