Given the equation $2H_2O ->2H_2 + O_2$, how many moles of $H_2O$ would be required to produce 2.5 moles of $O_2$?

Md Ariful Islam

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Md Ariful Islam

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Since the chemical equation,

$color(red)2H_2O->2H_2+color(blue)1O_2$

requires a specific number of moles of the reactant, then a specific number of moles of the products are created.

With this knowledge, you can create a mole ratio.

The general format of a mole ratio is as follows:

$color(blue)(|bar(ul(color(white)(a/a)color(black)(("required based on balanced equation")/("product based on balanced equation")=("required")/("product"))color(white)(a/a)|)))$

In your case, you're looking for the moles of $H_2O$ required to make $2.5$ moles of $O_2$.

Thus, your mole ratio would be:

$(color(red)2color(white)(i)molcolor(white)(i)H_2O)/(color(blue)1color(white)(i)molcolor(white)(i)O_2)=x/(2.5color(white)(i)molcolor(white)(i)O_2)$

$color(darkorange)(rArr)$where $x$ represents the moles of $H_2O$ required

From this point on, your goal is to solve for $x$ to find the moles of $H_2O$ required to produce $2.5$ moles of $O_2$.

$x=2.5color(purple)cancelcolor(black)(molcolor(white)(i)O_2)xx(2color(white)(i)molcolor(white)(i)H_2O)/(1color(purple)cancelcolor(black)(molcolor(white)(i)O_2))$

$x=color(green)(|bar(ul(color(white)(a/a)5color(white)(i)molcolor(white)(i)H_2Ocolor(white)(a/a)|)))$

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