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Standard XII

Chemistry

Introduction to Oxidation and Reduction

How much ener...

Question

How much energy will be released when $500 m l$ of $0.1 M$ of $H_{2} S O_{4}$ solution reacts with $1 L$ of $0.1 M$ $N H_{4} O H$ solution, if the base is $30 %$ ionized in the given solution?

5.75 kJ

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4.75

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5.15 kJ

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5.45 kJ

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Solution

The correct option is C 5.15 kJ
For neutralisation of 1 mole of hydrogen ions with 1 mole of hydroxide ions, 57.1 kJ of energy is released.
For the neutralisation of 1 mole of ammonium hydroxide with 0.5 moles of sulphuric acid, 51.5 kJ of energy is released as 5.6 kJ is required for the dissociation of ammonium hydroxide.
The number of moles of ammonium hydroxide present = $1 L \times 0.1 M = 0.1$ mol.
The energy released for 0.1 mole of ammonium hydroxide will be 5.15 kJ.

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Similar questions

Sulphuric acid reacts with sodium hydroxide as follows

$H_{2} S O_{4} + 2 N a O H \to N a_{2} S O_{4} + 2 H_{2} O$

When 1L of 0.1M sulphuric acid solutoin is allowed to react with 1L of 0.1M sodium hydroxide solutoin, the amount of sodium sulphate formed and its molarity in the solution obtained is ?

(a) $0.1 m o l L^{- 1}$ (b) $7.10 g$

Q. Which of the following solutions will be acidic?
(1)

0.1 M

F e {S O}_{4}

(2)

0.1 M

{({N H}_{4})}_{2} {S O}_{4}

(3)

0.1 M

{C H}_{3} C O O N a

(4)

0.1 M

{N H}_{4} O H

Q. Solution of

0.1 M

{N H}_{4} O H

and

0.1 M

{N H}_{4} C l

has pH

9.25

. Then

p K_{b}

{N H}_{4} O H

is:

Q. A

200

mL solution of

I_{2}

is divided into two unequal parts. Part I reacts with hypo solution in acidic medium and requires

8

mL of

2 M

hypo solution for complete neutralization.
Part II was added with

300

mL of

0.1 M

N a O H

solution. Residual base required

30

mL of

0.1 M

H_{2} S O_{4}

solution for complete neutralization. Calculate the value of

20

times the initial concentration of

I_{2}

Q. How many litres of

C O_{2}

at STP will be formed when

100 m l

0.1 M

H_{2} S O_{4}

reacts with excess of

N a_{2} C O_{3}

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How much energy will be released when 500ml of 0.1M of H2SO4 solution reacts with 1L of 0.1M NH4OH solution, if the base is 30% ionized in the given solution?

How much energy will be released when $500 m l$ of $0.1 M$ of $H_{2} S O_{4}$ solution reacts with $1 L$ of $0.1 M$ $N H_{4} O H$ solution, if the base is $30 %$ ionized in the given solution?