Question

The Volume of Oxygen ${\mathrm{O}}_2$liberated at STP when $100$ ml of $15$ Volume ${\mathrm{H}}_2{\mathrm{O}}_2$ decomposes is:

• A. $150$ml
• B. $300$ml
• C. $1500$ml
• D. $2000$ml

Answer 1

The correct option is C

$1500$ml

The Explanation for the Correct option

(c) $1500\mathrm{mL}$

${\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{liquid}\right)\stackrel{{\mathrm{MnO}}_2}{\to }{\mathrm{O}}_2\left(\mathrm{gas}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{liquid}\right)$

• It is a spontaneous decomposition of Hydrogen Peroxide $\left({\mathrm{H}}_2{\mathrm{O}}_2\right)$ into Water $\left({\mathrm{H}}_2\mathrm{O}\right)$ and Oxygen$\left({\mathrm{O}}_2\right)$.
• If$1$ ml of $15$ Volumes of${\mathrm{H}}_2{\mathrm{O}}_2$ liberates$15$ ml of Oxygen$\left({\mathrm{O}}_2\right)$.
• Then, $100$ml of $15$ Volumes of ${\mathrm{H}}_2{\mathrm{O}}_2$ liberates: $$\begin{gathered} =15\times 100 \\ =1500\mathrm{mL} \end{gathered}$$
• Hence, This Option is Correct.

The Explanation for the Incorrect options

Since, the correct volume is $1500\mathrm{mL}$. Therefore, options (a), (b) and (d) are incorrect.

Hence, The correct option is (c) $1500\mathrm{mL}$.