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

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

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

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

E M B I B E

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

MEDIUM

TS EAMCET

IMPORTANT

Earn 100

For a reaction $2 A ⇌ B + C, K_{c}$ is $2 \times 10^{- 3} .$ At a given time, the reaction mixture has $[A] = [B] = [C] = 3 \times 10^{- 4} M .$ Which of the following options is correct?

36.36% 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 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: