CameraIcon

SearchIcon

MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Stoichiometric Calculations

A sample of h...

Question

A sample of hydrazine sulphate $(N_{2} H_{6} S O_{4})$ was dissolved in $100$ mL water. $10$ mL of this solution was reacted with excess of $F e C l_{3}$ solution and warmed to complete the reaction. Ferrous ions formed was estimated and it required $20$ mL of $\frac{M}{50} K M n O_{4}$ solution. Estimate the mass of hydrazine sulphate in one litre of solution.
$4 F e^{3 +} + N_{2} H_{4} ⟶ N_{2} + 4 F e^{2 +} + 4 H^{+}$
$M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} ⟶ M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O$

A

6.5

g

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

B

2.5

g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

C

13

g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

3.5

g

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A $6.5$ g
The redox changes are given below:
$F e^{3 +} + e ⟶ F e^{2 +}$
$(N^{2 -})_{2} ⟶ N_{2}^{0} + 4 e$
$M n^{7 +} + 5 e ⟶ M n^{2 +}$
Meq. of $N_{2} H_{6} S O_{4} =$ Meq. of $F e C l_{3}$ reacting with $N_{2} H_{6} S O_{4} =$ Meq. of $F e^{2 +}$ formed $=$ Meq. of $K M n O_{4}$ used
Meq. of $N_{2} H_{6} S O_{4}$ in $10$ mL solution $=$ Meq. of $K M n O_{4}$ used $= 20 \times \frac{1}{50} \times 5 = 2$
$\frac{w}{\frac{M}{4}} \times 1000 = 2$ $⟹ \frac{w}{\frac{130}{4}} \times 1000 = 2$ (Molar mass of $N_{2} H_{6} S O_{4} = 130$ g/mol)
$w_{N_{2} H_{6} S O_{4}}$ in $10$ mL $= 0.065$ g
$∴ w_{N_{2} H_{6} S O_{4}}$ in $1000$ mL $= 6.5$ g/L

Suggest Corrections

thumbs-up

0

Similar questions

Q. A sample of hydrazine sulphate

(N_{2} H_{6} S O_{4})

was dissolved in

100 m L

10 m L

of this solution was reacted with an excess of

F e C l_{3}

solution and warmed to complete the reaction. Ferrous ion formed was estimated and it required

20 m L

\frac{M}{50} K M n O_{4}

. Estimate the amount of hydrazine sulphate in one litre of solution.
Reactions:

4 F e^{3 +} + N_{2} H_{4} \to N_{2} + 4 F e^{2 +} + 4 H^{+}

{M n O_{4}}^{-} + 5 F e^{2 +} + 8 H^{-} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

Q. A sample of hydrazine sulphate

(N_{2} H_{6} S O_{4})

was dissolved in

100

mL of water and

10

mL of this solution was reacted with excess of ferric chloride solution and warmed to complete the reaction. Ferrous ion formed was estimated and it required

20

\frac{M}{50}

potassium permanganate solution. Estimate the amount of hydrazine sulphate in

1

L of the solution. Reactions are given below:

4 F e^{3 +} + N_{2} H_{4} \to N_{2} + 4 F e^{2 +} + 4 H^{⨁}

M n O_{4}^{⊝} + 5 F e^{2 +} + 8 H^{⨁} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

A sample of hyhdrazine sulphate $(N_{2} H_{6} S O_{4})$ was dissolved in 100 ml water. 10 ml of this solution was reacted with excess of solution and warmed to complete the reaction. Ferrous ions formed required 20 ml of solution.
Given : $4 F e^{3 +} + N_{2} H_{4} \to N_{2} + F e^{2 +} + 4 H^{+}$
$M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O$

The amount (g) of hydrazine sulphate in one litre is

Q. 50 mL aqueous solution of

F e S O_{4}

required 12 mL of 0.2 M

K M n O_{4}

in acidic medium for complete oxidation. Calculate the molarity of ferrous sulphate solution. The reaction is:

M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

Q. Hydroxylamine reduces iron (III) according to the equation,

2 N H_{2} O H (a q) + 4 F e^{3 +} (a q) \to N_{2} O (g) ↑ + H_{2} O (l) + 4 F e^{2 +} (a q) + 4 H^{+} (a q)

Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is:

{M n O_{4}}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O

10 m L

sample of hydroxylamine solution was diluted to one litre.

50 m L

of this diluted solution was boiled with excess of iron (III) solution. The resulting solution required

12 m L

0.02 M K M n O_{4}

solution for complete oxidation of iron (II). Calculate the mass of hydroxylamine in one litre of the original solution.

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Stoichiometric Calculations

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Stoichiometric Calculations

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon