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Le Chatelier's Principle for Del N Equals to 0

Xg+Yg ⇌ ZgThe...

Question

$X (g) + Y (g) ⇌ Z (g)$
The diagram shows that the reaction between $X$ and $Y$ to form $Z$ had to equilibrium at time $t_{1}$ . The equilibrium shifts that occurred after time $t_{2}$ , were most likely caused by which of the following?

Adding more

X

and

Y

to the equilibrium mixture

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Adding more

X

to the equilibrium mixture

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Adding more

Y

to the equilibrium mixture

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Increasing temperature

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Increasing the pressure

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Solution

The correct option is A Adding more $X$ and $Y$ to the equilibrium mixture
We have seen in the graph that when we add more reactant in the equilibrium reaction the equilibrium shift to forward direction

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Similar questions

Q. At

550 K

K_{c}

for the reaction,

X (g) + Y (g) ⇋ Z (g)

, is

10^{4} m o l L^{- 1}

. At equilibrium it was observed that

[X]

\frac{1}{2} [Y]

\frac{1}{2} [Z]

. What is the value of

[Z]

m o l L^{- 1}

at equilibrium?

Q. At 550 K, the

K_{c}

for the following reaction is

10^{- 4} m o l^{- 1} l i t .

X (g) + Y (g) \Leftrightarrow Z (g) .

At equilibrium, it was observed that :

[X] = \frac{1}{2} [Y] = \frac{1}{2} [Z]

. What is the value of

[Z]

(

i n m o l l i t^{- 1}

) at equilibrium ?

Q. At 550 K, the

K_{c}

for the following reaction is

10^{4} m o l^{- 1} L : X (g) + Y (g) ⇌ Z (g)

. At equilibrium, it was observed that

[X] = \frac{1}{2} [Y] = \frac{1}{2} [Z]

.
What is the value of [Z]

(i n m o l L^{- 1})

at equilibrium?

Q. The equilibrium constant

K_{p}

of the reaction

X (g) ⇌ Y (g) + Z (g),

when

X (g)

decomposes to

50 %

at 5 atm pressure is:

Q. At

600^{\circ} C

K_{p}

for the following reaction is 1 atm

X (g) ⇌ Y (g) + Z (g)

. At equilibrium, 50% of X(g) is dissociated. The total pressure of the equilibrium system is P atm. What is the partial pressure (in atm) of X(g) at equilibrium ?

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X(g)+Y(g)⇌Z(g)The diagram shows that the reaction between X and Y to form Z had to equilibrium at time t1. The equilibrium shifts that occurred after time t2, were most likely caused by which of the following?

The correct option is A Adding more X and Y to the equilibrium mixtureWe have seen in the graph that when we add more reactant in the equilibrium reaction the equilibrium shift to forward direction

$X (g) + Y (g) ⇌ Z (g)$
The diagram shows that the reaction between $X$ and $Y$ to form $Z$ had to equilibrium at time $t_{1}$ . The equilibrium shifts that occurred after time $t_{2}$ , were most likely caused by which of the following?

The correct option is A Adding more $X$ and $Y$ to the equilibrium mixture
We have seen in the graph that when we add more reactant in the equilibrium reaction the equilibrium shift to forward direction