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help with stoichiometry problems?!?

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biricikelagozlum:
i need help balancing this equation and then answering a few questions.

Al + NaOH + H2O --> NaAlO2 + H2

a-) how many moles hydrogen can be produced from 16g Al?

b-) if 0.35 moles of hydrogen are actually produced, what is the % yield?

Mitch:
Al + NaOH + H2O --> NaAlO2 + (3/2)H2

Does that work?

Borek:
2Al + 2NaOH + 2H2O -> 2NaAlO2 + 3H2

Oh, how easy it is to use UBBC codes exported from EBAS ;)

And how easy it is to calculate soichiometry with EBAS ;)

Alberto_Kravina:

--- Quote ---Al + NaOH + H2O --> NaAlO2 + H2
--- End quote ---
I think that the oxo-aluminate hydrolizes to a hydroxo-aluminate complex since there is water involved in the reaction....

something like: Al + 3 H2O + NaOH ---> Na+ [Al(OH)4] - + 3/2 H2

...does anyone agree?

Borek:
I believe we can discuss this problem, to death, as the equilibrium is multistate. Still, there is 1.5 mole of H2 per mole of Al produced, and that's what counts for the OP question.

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