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In the explosion of a hydrogen-filled balloon, 0.10g of hydrogen reacted with 0.80g of...

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shelbyrob98 | Student, Grade 10 | eNoter

Posted August 22, 2013 at 2:00 AM via web

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In the explosion of a hydrogen-filled balloon, 0.10g of hydrogen reacted with 0.80g of oxygen. How many grams of water vapor are formed? (Water vapor is the only product.) How do i go about solving this? Thanks!

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llltkl | College Teacher | Valedictorian

Posted August 22, 2013 at 2:22 AM (Answer #1)

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Gaseous hydrogen reacts with oxygen to produce water according to the equation:

`2H_2+O_2 rarr 2H_2O`

The number of moles of the reactants are:

H2->0.1/2 =0.05

O2->0.8/32=0.025

according to the reaction stoichiometry,

2 moles of hydrogen require 1 mole of oxygen

so, 0.05 moles of hydrogen require 1*0.05/2, i.e. 0.025 moles of oxygen.

Exactly 0.025 moles of oxygen is present in the reaction mixture.

So, both the reactants would react and exhaust each other out.

From the balanced equation, 

2 moles of hydrogen reacts with sufficient oxygen to produce (2*+16), i.e. 18 g H2O

Therefore, 0.05 moles of hydrogen would produce 18*0.05/2, i.e. 0.45 g H2O.

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