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Question

10 g of Hydrogen and 64 g of Oxygen were filled in a steel vessel and exploded. Calculate the amount of water produced in the reaction.

A
2 mol
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B
5 mol
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C
3 mol
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D
4 mol
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Solution

The correct option is D 4 mol
Balanced reaction:
2H2+O22H2O

We know that, number of moles = Given massMolar mass

Number of moles of H2 = 102 = 5 mol

Number of moles of O2 = 6432 = 2 mol

We know that whenever moles of more than one reactant is given, we need to determine the limiting reagent (LR) in order to find the amount of product formed in the reaction.

Calculating LR,

For Hydrogen = number of molesstoichiometric coefficient = 52 = 2.5

For Oxygen = number of molesstoichiometric coefficient = 21 = 2

Since the above ratio is less for Oxygen, the limiting reagent will be Oxygen .

As per the stoichiometry, 1 mol of O2 produces 2 mol of H2O.
Hence, 2 mol of O2 will produce 4 mol of H2O.

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