Equilibrium C...

Equilibrium Constant and Standard Free Energy Change

Trending Questions

Q. Calculate

K_{p}

for the following reaction at

25^{\circ} C .

2 N_{2} O (g) ⇌ 2 N_{2} (g) + O_{2} (g)

Δ G_{f}^{0} (N_{2} O) = 104.2 k J / m o l, Δ G_{f}^{0} (N_{2}) = 0 a n d Δ G_{f}^{0} (O_{2}) = 0

$6.3 \times 10^{30}$
$3.3 \times 10^{36}$
$3.3 \times 10^{- 36}$
$6.3 \times 10^{- 30}$

View Solution

Q. Which of the following equilibriums degree of dissociation is independent of initial concentration?

$H I ⇌ \frac{1}{2} H_{2} + \frac{1}{2} I_{2}$
$P C l_{5} ⇌ P C l_{3} + C l_{2}$
$N_{2} O_{4} ⇌ 2 N O_{2}$
all the above

View Solution

Q. Calculate

△ G^{\circ}

for conversion of oxygen to ozone

3 / 2 O_{2} (g) \to O_{3} (g) a t 298 K, i f K_{p}

for this conversion is 2.47

\times

10^{- 29}

(Use log(2.47) = 0.4)

$163 K J m o l^{- 1}$
$2.4 X 10^{2} K J m o l^{- 1}$
$1.63 K J m o l^{- 1}$
$2.38 X 10^{6} K J m o l^{- 1}$

View Solution

Q. Which of the following chemical equilibria is favoured by increase in temperature?

$N_{2} O_{4} ⇌ 2 N O_{2} △ H = + 59 k J m o l^{- 1}$
$N_{2} + 3 H_{2} ⇌ 2 N H_{3} △ H = 22 k c a l m o l^{- 1}$
$2 S O_{2} + O_{2} ⇌ 2 S O_{3} △ H = 47 k c a l m o l^{- 1}$
All of the above

View Solution

Q. Consider the binding of oxygen to haemoglobin:

H b_{a q} + O_{2 (g)} ⇌ H b - O_{(a q)} .

If we decrease the pressure of the system, what is the effect on this equilibrium reaction?

The equilibrium shifts to the left
The equilibrium shifts to the right
There is no change in the system
None of the above

View Solution

Q. The equilibrium constant for the reaction in aqueous solution

H_{3} B O_{3} (a q) + g l y c e r i n (a q) ⇌ (H_{3} B O_{3} - g l y c e r i n) (a q) i s 0.90

.
How many moles of glycerin should be added per litre of

0.10 M H_{3} B O_{3}

so that

80 %

of the

H_{3} B O_{3}

is converted to the boric acid -glycerin complex?

$4.44$
$4.52$
$3.6$
$0.08$

View Solution

Q. The value of

Δ G^{\circ}

for a reaction having K=1 would be:

-RT
-1
\N
+RT

View Solution

For the reaction $N H_{4} H S_{(g)} ⇌ N H_{3 (g)} + H_{2} S_{(g)}$ in a closed flask, the equilibrium pressure is P atm. The standard free energy of the reaction would be :

-RT In p
-RT(In p - In 2)
-2 RT In p
-2 RT (In p - In 2)

View Solution

Q. Calculate

△ G^{\circ}

for conversion of oxygen to ozone

3 / 2 O_{2} (g) \to O_{3} (g) a t 298 K, i f K_{p}

for this conversion is 2.47

\times

10^{- 29}

(Use log(2.47) = 0.4)

$163 K J m o l^{- 1}$
$2.4 X 10^{2} K J m o l^{- 1}$
$1.63 K J m o l^{- 1}$
$2.38 X 10^{6} K J m o l^{- 1}$

View Solution

Q. For the reaction

2 A (g) + B (g) ⇌ C (g), △ H = + x k J,

Which of the following favour the formation of reactants?

Low pressure
High pressure
High temperature
Catalyst

View Solution

Q. Calculate

Δ_{r}

G for the reaction at

27^{\circ} C

H_{2} (g) + 2 A g^{+} (a q) ⇌ 2 A g (s) + 2 H^{+} (a q)

Given :

p_{H_{2}}

0.5 bar; [A g^{+}] = 10^{- 5} M; log 2 =0.3 log 2= 0.7

[H^{+}] = 10^{- 3} M; Δ_{r} G^{\circ} [A g^{+} (a q)] = 77.1 kJ/mol

$- 154.20 kJ/mol$
$- 178.90 kJ/mol$
$- 129.50 kJ/mol$
$+ 154.21 kJ/mol$

View Solution

Q. For the reaction

2 A (g) + B (g) ⇌ C (g), △ H = + x k J,

Which of the following favour the formation of reactants?

Low pressure
High pressure
High temperature
Catalyst

View Solution

Q. For the reaction,

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g), △ H = 57.49 {kJ mol}^{- 1}

.
With the increase in temperature, the vapour density of the equilibrium mixture:

Increases
Decreases
Remains the same
Can not be predicted

View Solution

Q. At equilibrium, reaction $A ⇋ B$ is at the stage of half completion. Which one of the followings is true?

$△ G^{\circ} = 0$
$△ G^{\circ} > 0$
$△ G^{\circ} < 0$
$△ G^{\circ} = - R T l n 2$

View Solution

Q. For the reaction

2 S O_{2} + O_{2} ⟶ 2 S O_{3}

if rate of disappearance of

O_{2}

is 8 g/s, then rate of appearance of

S O_{3}

will be:

16 g/s
4 g/s
40 g/s
10 g/s

View Solution

Q. The following reaction is performed at 298

K

2 N O (g) + O_{2} (g) ⇌ 2 N O_{2} (g)

The standard free energy of formation of

N O (g)

is 86.6 kJ/mol at 298 K. What is the standard free energy of formation of

N O_{2} (g)

at 298 K? (

K_{p} = 1.6 \times 10^{12}

)

R(298)ln( $1.6 \times 10^{12}$ ) - 86600
86600 + R(298)ln( $1.6 \times 10^{12}$ )
86600 - $\frac{l n (1.6 \times 10^{12})}{R (298)}$
0.5 [2 $\times$ 86600 - R(298)ln( $1.6 \times 10^{12}$ )

View Solution

The reaction N $_{2}$ O $_{4}$ (g) $⇌$ 2NO $_{2}$ (g) is
carried out at 298 K and 20 bar. Five moles of each of N $_{2}$ O $_{4}$ and
NO $_{2}$ , are taken initially. Given: $Δ$ $_{f}$ G $^{\circ}$
(N $_{2}$ O $_{4}$ ) = 100 kJ mol $^{- 1}$ and $Δ$ $_{f}$ G $^{\circ}$
(NO $_{2}$ ) = 50 kJ mol $^{- 1}$ .Choose the appropriate option: The values of
$Δ$ G and K $^{\circ}$ $_{p}$ at 298 K are:

$Δ$ G = 0, $K_{p}^{\circ}$ = 10 bar; The reaction is in equilibrium
5.7058 kJ $m o l^{- 1}$ , $K_{p}^{\circ}$ = 1 bar; The reaction goes in the reverse direction
-5.7058 kJ $m o l^{- 1}$ , $K_{p}^{\circ}$ = 1 bar; The reaction goes in the forward direction
$Δ$ G = 0, $K_{p}^{\circ}$ = 1 bar; The reaction is in equilibrium

View Solution

Q. Calculate the equilibrium concentration ratio of

C t o A

, if

2

moles each of

A

and

B

are allowed to come to equilibrium at

300 K

A (g) + B (g) ⇌ C (g) + D (g)

Δ G^{\circ} = - 1380 c a l / m o l

$0.56$
$4.45$
$1.50$
$3.16$

View Solution

Q. The equilibrium constant

K_{c}

for a reaction is 10. Calculate the value of change in standard Gibbs free energy

Δ G^{o} in k J m o l^{- 1}

at 300

K

5.744
-5.744
-2.744
2.744

View Solution

Q. Which of following graphs correctly depicts the variation of Gibbs Free Energy with extent of the Reaction ?

View Solution

Q. The standard free energy change of a reaction is

△ G^{o} = - 115 k J a t 298 K .

Calculate the equilibrium constant

K_{P}

l o g K_{P} . (R = 8.314 J K^{- 1} m o l^{- 1})

20.16
2.303
2.016
13.83

View Solution

Q. Which of the following is incorrect about the following reaction –
$2 S O_{2} (g) + O_{2} (g) ⇋ 2 S O_{3} (g) △ H = - 45 k C a l$

High pressure will be favorable for production of $S O_{3}$ .
High temperature will favor forward reaction.
Decreasing $S O_{3}$ concentration will reduce the rate of backward reaction.
Doubling the volume of container while keeping temperature same, will shift the equilibrium in reverse direction.

View Solution

Q. Calculate the equilibrium concentration ratio of

C t o A

, if

2

moles each of

A

and

B

are allowed to come to equilibrium at

300 K

A (g) + B (g) ⇌ C (g) + D (g)

Δ G^{\circ} = - 1380 c a l / m o l

$0.56$
$4.45$
$1.50$
$3.16$

View Solution

Q. For which of the following reactions at equilibrium at constant temperature doubling the volume will cause a shift to the right ( favour forward reaction)?

$N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$
$2 C O (g) + O_{2} ⇌ 2 C O_{2} (g)$
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$
All of these

View Solution

Q. Which of the following is incorrect about the following reaction –
$2 S O_{2} (g) + O_{2} (g) ⇋ 2 S O_{3} (g) △ H = - 45 k C a l$

High pressure will be favorable for production of $S O_{3}$ .
High temperature will favor forward reaction.
Decreasing $S O_{3}$ concentration will reduce the rate of backward reaction.
Doubling the volume of container while keeping temperature same, will shift the equilibrium in reverse direction.

View Solution

Q. The value of

Δ G^{\circ}

for a reaction having K=1 would be:

-RT
-1
\N
+RT

View Solution

Q. Value of

K_{p}

for the equilibrium reaction

$N_{2} O_{4 (g)} ⇌ 2 N O_{2 (g)}$ at 288 K is 47.9. The $K_{C}$ for this reaction at same temperature is ........(Nearest integer)

$(R = 0.083 L b a r K^{- 1} m o l^{- 1})$

 JEE MAIN 2021

View Solution