10g of hydrogen and 64g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:-(a) 3mol(b) 4mol(c) 1mol(d) 2 mol

To determine the amount of water produced in the reaction between hydrogen and oxygen, we need to calculate the limiting reactant first. The limiting reactant is the one that is completely consumed and determines the maximum amount of product that can be formed.

Let's start by converting the given masses of hydrogen and oxygen into moles using their respective molar masses:

Molar mass of hydrogen (H₂) = 2 g/mol
Molar mass of oxygen (O₂) = 32 g/mol

Number of moles of hydrogen (H₂) = mass of hydrogen / molar mass of hydrogen
= 10 g / 2 g/mol
= 5 mol

Number of moles of oxygen (O₂) = mass of oxygen / molar mass of oxygen
= 64 g / 32 g/mol
= 2 mol

From the balanced chemical equation for the reaction:

2H₂ + O₂ → 2H₂O

We can see that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.

However, we have 5 moles of hydrogen and only 2 moles of oxygen. Since the oxygen is the limiting reactant, we can only form a maximum of 2 moles of water.

Therefore, the correct option is (d) 2 mol.