K_p = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C₂H₆ when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

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Solution

Let p be the pressure exerted by ethene and hydrogen gas (each) at equilibrium.

Now, according to the reaction,

We can write,

Hence, at equilibrium,

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K_p = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C₂H₆ when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

$K_{p} = 0.04$ atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of $C_{2} H_{6}$ when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?
$C_{2} H_{6} (g) \leftrightarrow C_{2} H_{4} (g) + H_{2} (g)$

K_{P} = 0.04

atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of

C_{2} H_{6}

when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

C_{2} H_{6} (g) ⇌ C_{2} H_{4} (g) + H_{2} (g)

K_{p} = 0.04 a t m

at 899 K for the equilibrium shown below. What is the equilibrium concentration of

C_{2} H_{6}

when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

C_{2} H_{6} (g) ⇌ C_{2} H_{4} (g) + H_{2} (g)

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Kp = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C2H6 when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

Let p be the pressure exerted by ethene and hydrogen gas (each) at equilibrium. Now, according to the reaction, We can write, Hence, at equilibrium,

K_p = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C₂H₆ when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?

Let p be the pressure exerted by ethene and hydrogen gas (each) at equilibrium.

Now, according to the reaction,

We can write,

Hence, at equilibrium,