Question

A chemist pumps hydrogen gas (H2) from a tank into a reaction vessel containing 0.734 mol O2. The gases react to form water. If all of the available O2 reacts, how many moles of H2 are used?

Answer 1

2H2+O2 ----> 2H2O

Therefore, 2 mol of H2 react with 1 mole of O2. Therefore, to react with 0.734mol of O2, we need 2×0.734mol = 1.468 mol of H2.

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Answer 2

1.468 moles of $H_2$ are used.

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

The balanced chemical reaction for formation of water is:

$2H_2+O_2\rightarrow 2H_2O$

According to stoichiometry:

1 mole of oxygen  $(O_2)$ uses = 2 mole of hydrogen $(H_2)$

0.734 mole of oxygen  $(O_2)$ uses = $\frac{2}{1}\times 0.734=1.468$ mole of hydrogen $(H_2)$

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