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
Answers
Explanation:
both b and c are correct .
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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.