NEET Kp, Kc & Factors Affecting them Practice Questions With Solutions

NEET Chemistry Kp, Kc & Factors Affecting them Practice Questions

Question 1.

For the reaction $A(g) \rightleftharpoons 2B(g),$ the backward reaction rate constant is higher than the forward reaction rate constant by a factor of $2500$ at $1000~K $.$K_p$ for the reaction at $1000~ K$ is: [ Given: ${R= 0.0831~ L ~\text{atm mol}^{-1} }K^{-1}]$

A$0.033 $

B$0.021 $

C$83.1 $

D$2 .077 \times 10^5$

Question 2.

Consider the reaction in equilibrium $\mathrm{PCl}_5=\mathrm{PCl}_3+\mathrm{Cl}_2$ at $500 \mathrm{~K} .$ The concentration of $\mathrm{PCl}_5=1.40~ \mathrm{M} \text {, }$ concentration of $\mathrm{Cl}_2=1.60~ \mathrm{M} \text {, }$ concentration of $\mathrm{PCl}_3=1.60 \mathrm{M}$. Calculate $K_c$:

B2.6

C1.83

D3.4

Question 3.

In which of the following equilibria, $\text{K}_\text{p}$ and $\text{K}_\text{c}$ are NOT equal?

A$\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}_{(\mathrm{g})}$

B$\mathrm{CO}_{(\mathrm{g})}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}$

C$2 \mathrm{BrCl}_{(\mathrm{g})} \rightleftharpoons \mathrm{Br}_{2(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}$

D$\mathrm{PCl}_{5(\mathrm{~g})} \rightleftharpoons \mathrm{PCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})}$

Question 4.

A 20-litre container at 400 K contains CO₂ (g) at pressure 0.4 atm and an excess of SrO (neglecting the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container.
The maximum volume of the container, when the pressure of CO₂ attains its maximum value will be:
(Given that: SrCO₃(s) ⇋ SrO(s) + CO₂(g) , Kp = 1.6 atm)

A10 litre

B2 litre

C4 litre

D5 litre

Question 5.

The value of the equilibrium constant for a particular reaction is 1.6 × 10¹². When the system is in equilibrium, it will include:

AAll reactants

BMostly reactants

CMostly products

DSimilar amounts of reactants and products

Question 6.

If the equilibrium constant for N₂(g) + O₂(g)⇄ 2NO(g) is K, the equilibrium constant for$\frac{1}{2}$N₂(g) + $\frac{1}{2}$O₂(g) ⇄ NO(g) will be?

K^{\frac{1}{2}}

\frac{1}{2} K

K^{2}

Question 7.

The equilibrium reaction that doesn't have equal values for K_c and K_pis:

A$2NO(g) \rightleftharpoons N_2(g) + O_2(g)$

B$SO_2(g) + NO_2(g) \rightleftharpoons SO_3(g) + NO(g)$

C$H_2(g) + I_2(g) \rightleftharpoons 2HI (g)$

D$2C(s) + O_2(g) \rightleftharpoons 2CO_2(g)$

Question 8.

The dissociation constants for acetic acid and HCN at 25 °C are 1.5 x 10^-5and 4.5 x 10^-10, respectively. The equilibrium constant for the equilibrium, CN^- + CH₃COOH ⇌ HCN + CH₃COO^- would be:

3.0 \times 10^{5}

3.0 \times 10^{- 5}

3.0 \times 10^{- 4}

3.0 \times 10^{4}

Question 9.

The dissociation equilibrium of a gas AB₂ can be represented as $2 A B_{2} (g)$ $⇋$ $2 A B (g)$ $+$ $B_{2} (g)$ The degree of dissociation is ‘x’ and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant K_P and total pressure p is:

A(2KP/p)

B(2Kp /p)^1/3

C(2KP/p)^1/2

D(KP/P)

Question 10.

The value of K_P1 and K_p2 for the reactions

X

⇋

Y

+ Z

. . . . . . (i)

a n d

A

⇋ 2 B

. . . . . . (i i)

are in the ratio of 9 : 1. If the degree of dissociation of X and A is equal, then the total pressure at equilibrium(i) and (ii) are in the ratio:

A3 : 1

B1 : 9

C36 : 1

D1 : 1

Question 1.

The value of the equilibrium constant of the reaction

HI (g)

⇋

\frac{1}{2} H_{2} (g)

+

\frac{1}{2} I_{2}

is 8.0.
The equilibrium constant of the reaction

H_{2} (g)

+

I_{2} (g)

⇋

2 HI (g)

will be-

A$1 \over 16$

B$1 \over 64$

C16

D$1 \over 8$

Question 2.

The following equilibrium constants are given:
N₂ + 3H₂ ⇌ 2NH₃; K₁
N₂ + O₂⇌ 2NO; K₂
H₂ + 1/2O₂ ⇌ H₂O; K₃

The equilibrium constant for the oxidation of NH₃ by oxygen to give NO is:

K_{2} K_{3}^{3} / K_{1}

K_{2} K_{3}^{2} / K_{1}

K_{2}^{2} K_{3} / K_{1}

K_{1} K_{2} / K_{3}

Question 3.

For the reaction,
CH₄(g) + 2O₂(g)

CO₂(g) + 2H₂O(l)
Δ_rH = -170.8 kJ mol^-1
Which of the following statements is not true?

AAt equilibrium, the concentration of $\mathrm{CO}_2 \mathrm{~g}$ and water (l) are not equal.

BThe equilibrium constant for the reaction is given by $K_p=\frac{\left[\mathrm{CO}_2\right]}{\left[\mathrm{CH}_4\right]\left[\mathrm{O}_2\right]}$

CThe addition of $\mathrm{CH}_4 \mathrm{~g} $ or $\mathrm{O}_2 \mathrm{~g}$ at equilibrium will cause a shift to the right

DThe reaction is exothermic

Question 4.

For a reaction ,

{BaO}_{2} (s) ⇌ BaO (s) + O_{2} (g)

; ∆H = + ve. At equilibrium condition, the pressure of O₂ depends on the:

AIncreased mass of BaO₂

BIncreased mass of BaO

CIncreased temperature onequilibrium.

DIncreased mass of BaO₂ and BaO both.

Question 5.

The ionization constant of $CH_{3} COOH$ is 1.7 × $\left(10\right)^{- 5}$ and the concentration of $H^{+ }$ions is 3.4 × $\left(10\right)^{- 4}$. The initial concentration of $CH_{3} COOH$ will be:

A3.4 × $\left(10\right)^{- 4}$

B3.4× $\left(10\right)^{- 3}$

C6.8 × $\left(10\right)^{- 4}$

D6.8 × $\left(10\right)^{- 3}$

Question 6.

For any reversible reaction, if we increase the concentration of the reactants, the effect on equilibrium constant will:

ADepend on the amount of concentration

BRemain unchanged

CDecrease

DIncrease

Question 7.

The correct relation between dissociation constants of a di-basic acid is:

K a_{1} = K a_{2}

K a_{1} > K a_{2}

K a_{1} < K a_{2}

K a_{1} = \frac{1}{K a_{2}}

Question 8.

Given the following two reactions:
A + B ⇌ C + D, with rate constant K₁
E + F ⇌ G + H, with rate constant K₂ If C + D + E + F produces a product, what is the rate constant for this reaction?

A$\dfrac{K_1}{K_2}$

B$\dfrac{K_2}{K_1}$

C$K_1K_2$

DNone of the above

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NEET Kp, Kc & Factors Affecting them Practice Questions With Solutions

NEET Chemistry Kp, Kc & Factors Affecting them Practice Questions

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

Question 10.

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

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