Question

Urgent....Calculate the amount of H2 which is unreacted in the given reaction 2H2+O2=2H2O...if 8g of H2 is react with 16 g of O2...

Answer 1

Answer: 3 moles

Explanation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Moles of $H_2$

[tex]\text{Number of moles of hydrogen}=\frac{8g}{2g/mol}=4moles [/tex]

Moles of [tex]O_2 [/tex]

[tex]\text{Number of moles of oxygen}=\frac{16g}{32g/mol}=0.5moles [/tex]

For the given balanced chemical equation:

$2H_2+O_2\rightarrow 2H_2O$

By Stoichiometry:

1 mole of oxygen reacts with 2 mole of  hydrogen

So, 0.5 moles of oxygen react with = $\frac{2}{1}\times 0.5=1.0$ mole of  hydrogen

Oxygen is considered as a limiting reagent because it limits the formation of product and  is the excess reagent.Hydrogen is the excess reagent and (4-1)= 3 moles of hydrogen will remain unreacted.

Answer 2

Answer:

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Explanation:

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