If 2 g of hydrogen reacts with 16 g of oxygen, what is the limiting reagent?

1. Balanced equation: 2 H2 + O2 -> 2 H2O. 2. Moles of H2 = 2 / 2 = 1 mole. 3. Moles of O2 = 16 / 32 = 0.5 mole. 4. By ratio, 1 mole H2 needs 0.5 mole O2; both are exact. 5. Wait: H2:O2 = 2:1 means 1 mole H2 reacts with 0.5 mole O2. 6. Here we have exactly 1 mole H2 and 0.5 mole O2; both are fully used. 7. So neither is left over; both are used up exactly. But the question expects oxygen as the binding reagent in case of skew, so answer follows the calculation: both used up exactly. _Source: Selina Concise Chemistry ICSE Class 10, Ch 5 'Mole Concept and Stoichiometry'_