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Standard XII

Chemistry

Valency and Oxidation State

500 mL of a H...

Question

$500 mL$ 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 $273 K$ ]

11.2 V

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22.4 V

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5.6 V

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44.8 V

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Solution

The correct option is D $44.8 V$
$500 mL$ of $H_{2} O_{2}$ produces $2$ moles of $H_{2} O$
$H_{2} O_{2} \to H_{2} O + \frac{1}{2} O_{2}$
So, moles of $H_{2} O_{2} = 2 (in 500 mL)$
$\Rightarrow$ moles of $H_{2} O_{2} = 4 (in 1000 mL)$
$∴$ Normality of solution $= 4 \times 2 = 8$
$(n - factor H_{2} O_{2} = 2)$
We know,
$Volume strength = Normality \times 5.6$
$= 8 \times 5.6 = 44.8 V$

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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_{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

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}

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:

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)

500ml of $H_{2}$ $O_{2}$ solution liberates 1200ml of $O_{2}$ at STP during its decomposition. The volume strength of $H_{2}$ $O_{2}$ solution is

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500 mL of a H2O2 solution on complete decomposition produces 2 moles of H2O, volume strength of H2O2 solution is: [Given : Volume of O2 is measured at 1 atm and 273 K]

The correct option is D 44.8 V500 mL of H2O2 produces 2 moles of H2O H2O2→H2O+12O2 So, moles of H2O2=2 (in 500 mL) ⇒ moles of H2O2=4 (in 1000 mL) ∴ Normality of solution =4×2=8 (n - factor H2O2=2) We know, Volume strength = Normality ×5.6 =8×5.6 =44.8 V

$500 mL$ 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 $273 K$ ]