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Standard XII

Chemistry

Le Chatelier's Principle for Del N Equals to 0

500 ml of a ...

Question

$500$ ml of a $H_{2} O_{2}$ solution on complete decomposition produces $2$ moles of $H_{2} O_{2}$ . Calculate the volume strength of $H_{2} O_{2}$ solution?
[Assume that the volume of $O_{2}$ is measured at $1$ atm and $273$ K]

44.8 V

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45.6 V

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49.3 V

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54.7 V

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Solution

The correct option is A $44.8 V$
As we know, volume strength of $H_{2} O_{2} = 5.6 \times N o r m a l i t y$ .

Here, $500 m l$ solution produces $2$ moles of $H_{2} O_{2}$

So, one litre will produce $4$ moles of $H_{2} O_{2}$ .

Therefore, normality of solution $= 4 \times 2 = 8$

$∴$ $n - f a c t o r$ of $H_{2} O_{2}$ is $2$

Therefore, volume strength of $H_{2} O_{2} = 5.6 \times 8 = 44.8 V$ .

Hence, option $A$ is correct.

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Similar questions

500 mL

of a

H_{2} O_{2}

solution on complete decomposition produces

2

moles of

H_{2} O

, volume strength of

H_{2} O_{2}

solution is:
[Given : Volume of

O_{2}

is measured at

1 atm

and

273 K

]

Q. The srength of

H_{2} O_{2}

is expressed in several ways like molarity, normality, %(w/V), volume strength, etc. The strength of

10 V

means 1 volume of

H_{2} O_{2}

on decomposition gives 10 volumes of oxygen at 1 atm and

273 K

or 1 litre of

H_{2} O_{2}

gives

10 l i t r e

O_{2}

at 1 atm and

273 K

.
The decomposition of

H_{2} O_{2}

is shown as under:

H_{2} O_{2} (a q) \to H_{2} O (l) + \frac{1}{2} O_{2} (g)

H_{2} O_{2}

can acts as oxidising as well as reducing agent, as oxidisng agent

H_{2} O_{2}

converted into

H_{2} O

and as reducing agent

H_{2} O_{2}

converted into

O_{2}

, both cases n-factor is

2

∴, Normality of H_{2} O_{2} Solution = 2 \times Molarity of H_{2} O_{2} Solution

What is the percentage strength of

11.2 V H_{2} O_{2}

Q. 44.8 V

H_{2} O_{2}

Solution (500 ml) when exposed to atmosphere looses 11.2 litre of

O_{2}

at 1 atm & 273K. New molarity of

H_{2} O_{2}

solution (Assume no change in volume)

Q. .............. volume

H_{2} O_{2}

solution means that

1

mL of

H_{2} O_{2}

at NTP gives

1

L of

O_{2}

10

mL of a solution of

H_{2} O_{2}

requires

25

mL of

0.1

K M n O_{4}

for complete reaction. The volume strength of

H_{2} O_{2}

is:

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500 ml of a H2O2 solution on complete decomposition produces 2 moles of H2O2. Calculate the volume strength of H2O2 solution? [Assume that the volume of O2 is measured at 1 atm and 273 K]

$500$ ml of a $H_{2} O_{2}$ solution on complete decomposition produces $2$ moles of $H_{2} O_{2}$ . Calculate the volume strength of $H_{2} O_{2}$ solution?
[Assume that the volume of $O_{2}$ is measured at $1$ atm and $273$ K]