Question

1 g of hydrogen reacts with 8 g of oxygen to produce 9 g of water.
 Select the correct option when 20 g of oxygen reacts with 3 g of hydrogen-
a)23 g of water will be produced.
b)22.5 g of water will be produced
c)22.5 g of water will be produced and 0.5 g of hydrogen will remain unreacted
d)Both b and c
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Answer 1

Explanation:

both b and c are correct .

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Answer 2

The balanced chemical equation for the reaction is :-

2H₂ + O₂ → 2H₂O

Here, we are given with 20g of O₂ and 3g of H₂.

Number of moles in 3g H₂ :-

= Given Mass/Molar mass

= 3/2

= 1.5 mole

Number of moles in 20g O₂ :-

= Given Mass/Molar mass

= 20/32

= 0.625 mole

According to the balanced equation , 2 mole of H₂ reacts with 1 mole of O₂.

Thus, 1.5 mole of H₂ will react with :-

= 1.5/2

= 0.75 mole of O₂.

Here, we are given with more moles of H₂ than O₂. Thus, 0.625/2 = 1.25 mole of H₂ will react and remaining 0.25 mole will remain unreacted.

O₂ is the limiting reagent and will control the amount of product.

Now, again according to the balanced equation :-

∵ 32g O₂ → 36g H₂O

∴ 20g O₂ → 20×36/32 = 22.5g H₂O

Mass of H₂ that remains unreacted :-

= No of mole × Molar mass

= 0.25 × 2

= 0.5g

_______________________________

Thus, mass of water formed is 22.5g and 0.5g of hydrogen remains unreacted.

Hence, Option.D is correct.