Question

$100c{m^3}$ of a given sample of ${H_2}{O_2}$ gives $1000 \;c{m^3}$ of ${O_2}$ at S.T.P. the given sample is:
A) $10% {H_2}{O_2}$
B) $90% {H_2}{O_2}$
C) $10$ volume ${H_2}{O_2}$
D) $100$ volume ${H_2}{O_2}$

Answer 1

Hint: Hydrogen peroxide is a chemical compound with the formula ${H_2}{O_2}$. ${H_2}{O_2}$ on catalytic Decomposition breaks down to give molecules of water and oxygen ${H_2}$ and ${O_2}$.

Complete answer:
Decomposition is catalysed by various transition metals and their compounds. It is highly unstable in nature and it is stored with a stabilizer in a weakly acidic solution in a dark colored bottle.
he decomposition reaction of ${H_2}{O_2}$ is:
\[{H_2}{O_2} \to {H_2}O + \dfrac{1}{2}{O_2}\]
$\dfrac{1}{2}$ mole of ${O_2}$ is obtained from $34\;g\;{H_2}{O_2}$ .
$1$ ml of ${H_2}{O_2}$ will give $10$ml from ${O_2}$ at STP
10 volume’ means that 10 $cm^3$ of oxygen gas is produced by every 1 $cm^3$ of hydrogen peroxide. Thus for every $100c{m^3}$ the oxygen liberated is $1000c{m^3}$. The sample of ${H_2}{O_2}$ which will be required is
\[\dfrac{{1oooc{m^3}}}{{100c{m^3}}} = 10c{m^3}\]
Hence for the $1000c{m^3}$ of ${O_2}$ 10 times the volume of the sample is required.

Therefore the correct option is option (C) .

Additional Information: Hydrogen peroxide has been used as a propellant in rockets and torpedoes. This is because the decomposition reaction can be speeded up greatly by adding a catalyst. Producing a large volume of gas in a short time and small space creates a lot of energy.

Note: The reaction happens slowly while hydrogen peroxide is stored, because unevenness in the container’s surface can help to split the molecule – one part gets stuck to the surface while the other part pulls away.