For a reaction 2 A ⇌ B + C , K c is 2 × 10 - 3 . At a given time, the reaction mixture has [ A ] = [ B ] = [ C ] = 3 × 10 - 4 M . Which of the following options is correct?

The reaction proceeds to the left

The reaction proceeds to the right

Following lists contain reactions and their corresponding equilibrium constants at different temperatures: List - I (Reaction) List - II K p 2 SO 2 ( g ) + O 2 ( g ) ⇌ 2 SO 3 ( g ) at 298 K 4 . 0 × 10 24 2 SO 2 ( g ) + O 2 ( g ) ⇌ 2 SO 3 ( g ) at 700 K 3 . 0 × 10 4 N 2 O 4 ( g ) ⇌ 2 NO 2 ( g ) at 298 K 0 . 98 N 2 O 4 ( g ) ⇌ 2 NO 2 ( g ) at 500 K 1700 If ∆ H 1 0 and ∆ H 2 0 are the standard enthalpies for the reactions 2 SO 2 + O 2 ⇌ 2 SO 3 and N 2 O 4 ⇌ 2 NO 2 respectively, then:

∆ H 1 0 is negative and ∆ H 2 0 is positive

Both ∆ H 1 0 and ∆ H 2 0 are negative

Both ∆ H 1 0 and ∆ H 2 0 are positive

∆ H 1 0 is positive and ∆ H 2 0 is negative

For a reaction 2 A ⇌ B + C , K c is 2 × 10 - 3 . At a given time, the reaction mixture has [ A ] = [ B ] = [ C ] = 3 × 10 - 4 M . Which of the following options is correct?

The reaction proceeds to the left

The reaction proceeds to the right

Following lists contain reactions and their corresponding equilibrium constants at different temperatures: List - I (Reaction) List - II K p 2 SO 2 ( g ) + O 2 ( g ) ⇌ 2 SO 3 ( g ) at 298 K 4 . 0 × 10 24 2 SO 2 ( g ) + O 2 ( g ) ⇌ 2 SO 3 ( g ) at 700 K 3 . 0 × 10 4 N 2 O 4 ( g ) ⇌ 2 NO 2 ( g ) at 298 K 0 . 98 N 2 O 4 ( g ) ⇌ 2 NO 2 ( g ) at 500 K 1700 If ∆ H 1 0 and ∆ H 2 0 are the standard enthalpies for the reactions 2 SO 2 + O 2 ⇌ 2 SO 3 and N 2 O 4 ⇌ 2 NO 2 respectively, then:

∆ H 1 0 is negative and ∆ H 2 0 is positive

Both ∆ H 1 0 and ∆ H 2 0 are negative

Both ∆ H 1 0 and ∆ H 2 0 are positive

∆ H 1 0 is positive and ∆ H 2 0 is negative

EASY

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IMPORTANT

Earn 100

For the given equilibrium reaction,
$2 A (g) ⇌ 2 B (g) + C (g)$
the equilibrium constant $(K_{c})$ at $1000 K$ is $4 \times 10^{- 4}$ . Calculate $K_{p}$ for the reaction at $800 K$ temperature

76.47% studentsanswered this correctly

Important Questions on Chemical Equilibrium

MEDIUM

TS EAMCET

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 7 - Chemical Equilibrium>TS EAMCET 2018 (04-May Shift-1)>Q 3

For a reaction

2 A_{(g)} ⇌ 2 B_{(g)} + C_{(g)}, K_{c} = 3.75 \times 10^{- 6}

1069 K

. The approximate value of

K_{p}

for this reaction at the same temperature is

(R = 0.082 L bar {mol}^{- 1} K^{- 1})

HARD

TS EAMCET

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 7 - Chemical Equilibrium>TS EAMCET 2021 (04-Aug Shift-2)>Q 4

For the reaction

A_{(g)} ⇌ B_{(g)} + C_{(g)}, A

33 %

dissociated at a total pressure

P .

The correct relation between

P

and

K_{p}

MEDIUM

TS EAMCET

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 7 - Chemical Equilibrium>TS EAMCET 2021 (04-Aug Shift-2)>Q 5

The value of the reactant quotient

(\emptyset)

for the cell is

Zn (s) / {Zn}^{2 +} (0.01 M) ‖ {Cu}^{2 +} (1.25 M) / Cu (s)

MEDIUM

TS EAMCET

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 7 - Chemical Equilibrium>TS EAMCET - 5 August 2021 Shift 1>Q 6

For a reaction

2 A ⇌ B + C, K_{c}

2 \times 10^{- 3} .

At a given time, the reaction mixture has

[A] = [B] = [C] = 3 \times 10^{- 4} M .

Which of the following options is correct?

MEDIUM

TS EAMCET

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 7 - Chemical Equilibrium>TS EAMCET 2019 (03-May Shift-2)>Q 7

Following lists contain reactions and their corresponding equilibrium constants at different temperatures:

List - I (Reaction)	List - II $(K_{p})$
$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g) at 298 K$	$4.0 \times 10^{24}$
$2 {SO}_{2} (g) + O_{2} (g) ⇌ 2 {SO}_{3} (g) at 700 K$	$3.0 \times 10^{4}$
$N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g) at 298 K$	$0.98$
$N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g) at 500 K$	$1700$

If $∆ H_{1}^{0} and ∆ H_{2}^{0}$ are the standard enthalpies for the reactions $2 {SO}_{2} + O_{2} ⇌ 2 {SO}_{3} and N_{2} O_{4} ⇌ 2 {NO}_{2}$ respectively, then:

HARD

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IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 7 - Chemical Equilibrium>TS EAMCET - 5 August 2021 Shift 1>Q 8

The equilibrium constant

(K_{p})

for the formation of ammonia from its constituent elements at

27 ° C

1.2 \times 10^{- 4}

and at

127 ° C

0.60 \times 10^{- 4} .

Calculate the mean heat of formation of ammonia per mole in this temperature range.

MEDIUM

TS EAMCET

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 7 - Chemical Equilibrium>TS EAMCET 2018 (04-May Shift-1)>Q 9

298 K

, the equilibrium constant of the process

1.5 O_{2 (g)} ⇌ O_{3 (g)}

3 \times 10^{- 29}

. Standard free energy change (in

kJ {mol}^{- 1}

) of the process is approximately

(R = 8.314 J {mol}^{- 1} K^{- 1}; \log 3 = 0.47)

For the given equilibrium reaction, 2 Ag⇌2 Bg+Cg the equilibrium constant Kc at 1000 K is 4×10-4. Calculate Kp for the reaction at 800 K temperature

Important Questions on Chemical Equilibrium

Learn and Prepare for any exam you want !

For the given equilibrium reaction,
$2 A (g) ⇌ 2 B (g) + C (g)$
the equilibrium constant $(K_{c})$ at $1000 K$ is $4 \times 10^{- 4}$ . Calculate $K_{p}$ for the reaction at $800 K$ temperature