Question

10g of hydrogen and 64g of oxygen were filled in a steel vessel and exploded. The amount of water produced in this reaction will be____________.

• A. 2 mole
• B. 3 mole
• C. 4 mole
• D. 1 mole

Answer 1

The correct option is C

4 mole

$\underset{\mathrm{Hydrogen}}{2{\mathrm{H}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{Oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Water}}{2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}$

4-gram Hydrogen reacts with 32 grams of oxygen to produce 36 grams of water.

$\frac{4}{32}\mathrm{gram}$ Hydrogen reacts with $\frac{32}{32}\mathrm{gram}$ oxygen to produce $\frac{36}{32}\mathrm{gram}$ water.

$64\times \frac{4}{32}\mathrm{gram}$ Hydrogen reacts with $64\times \frac{32}{32}\mathrm{gram}$ oxygen to produce $64\times \frac{36}{32}\mathrm{gram}$ water.

$8\mathrm{gram}$ Hydrogen reacts with $64\mathrm{gram}$ oxygen to produce $\mathit{72}\mathit{}\mathrm{gram}$ water.

Oxygen is a limiting reagent here.

Mole of substance=$\frac{\mathrm{Given}\mathrm{mass}\mathrm{of}\mathrm{the}\mathrm{substance}}{\mathrm{Molecular}\mathrm{mass}\mathrm{of}\mathrm{the}\mathrm{substance}}$

Moles of produced water$\frac{72}{18}=4\mathrm{mole}$

Hence, Option(C) is correct.