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System, Surroundings, Intensive, Extensive Properties

Enthalpy of d...

Question

Enthalpy of dissociation of (in $k J m o l^{- 1}$ ) of acetic acid obtained from Expt. 2 is:

A

1

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B

10

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C

24.5

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D

51.4

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Solution

The correct option is A 1
$H C l + N a O H \to N a C l + H_{2} O$
100 m.mol 100 m.mol - -
- - 100 m.mol 100 m.mol
$Q = + 57 \times 1000 \times \frac{100}{1000} = [200 \times 4.2 + C] \times 5.7$ .......(1)
$C H_{3} C O O H + N a O H \to C H_{3} C O O N a + H_{2} O$
200 100 - -
100 - 100 -
$| Δ H | \times 1000 \times \frac{100}{1000} = [200 \times 4.2 + C] \times 5.6$ ........(2)
By equation 1 and 2,
$⟹ | Δ H | = 56$
$⟹ Δ H_{n e u t r a l i s a t i o n} = - 56 k J / m o l$
Now,
$⟹ - 56 = - 57 + Δ H_{I E}$
$⟹ Δ H_{I E} = 1 k J / m o l$

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Similar questions

m L

M

H C l

was mixed with 100

m L

M

N a O H

in an insulated beaker at constant pressure, a temperature increase of

{5.7}^{\circ} C

was measured for the beaker and its contents (Expt 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0

k J m o l^{- 1}

), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt 2), 100

m L

M

(K_{a} = 2.0 \times 10^{- 5})

was mixed with 100

m L

M

N a O H

(under identical conditions to Expt 1) where a temperature rise of

{5.6}^{\circ} C

was measured.
(Consider heat capacity of all solutions as

4.2 J g^{- 1} K^{- 1}

and density of all solutions as

1.0 g m L^{- 1}

)

Enthalpy of dissociation (in

k J

m o l^{- 1}

) of acetic acid obtained from the Expt. 2 is:

m L

M

H C l

was mixed with 100

m L

M

N a O H

in an insulated beaker at constant pressure, a temperature increase of

{5.7}^{\circ} C

was measured for the beaker and its contents (Expt 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0

k J m o l^{- 1}

), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt 2), 100

m L

M

(K_{a} = 2.0 \times 10^{- 5})

was mixed with 100

m L

M

N a O H

(under identical conditions to Expt 1) where a temperature rise of

{5.6}^{\circ} C

was measured.
(Consider heat capacity of all solutions as

4.2 J g^{- 1} K^{- 1}

and density of all solutions as

1.0 g m L^{- 1}

)

Enthalpy of dissociation (in

k J

m o l^{- 1}

) of acetic acid obtained from the Expt. 2 is:

Q. Calculate the lattice enthalpy of

K C l

from the following data at standard states-
Enthalpy of sublimation of

K = 89 k J m o l^{- 1}

Enthalpy of dissociation of

C l_{2} = 244 k J m o l^{- 1}

Ionisation energy of

K = 425 k J m o l^{- 1}

Electron gain enthalpy of

C l = - 355 k J m o l^{- 1}

Enthalpy of formation of

K C l = - 438 k J m o l^{- 1}

Q. Bond dissociation enthalpies of

H_{2} (g) a n d N_{2} (g)

436.0 k J m o l^{- 1}

941.3 k J m o l^{- 1}

respectively. Enthalpy of formation of

N H_{3}

- 46.0 k J m o l^{- 1}

. What is the enthalpy of atomization of

N H_{3}

.

Q. Calculate the enthalpy of formation of acetic acid (

C H_{3} C O O H

) if its enthalpy of combustion is

- 867 k J m o l^{- 1}

.The enthalpies of formation of

C O_{2} (g)

H_{2} O (l)

- 285.9 k J m o l^{- 1}

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