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Le Chatelier's Principle for Del N Greater Than Zero

Thermal decom...

Question

Thermal decomposition of gaseous $X_{2}$ to gaseous X at 298 K takes place according to the following equation:
$X_{2} (g) ⇌ 2 X (g)$
The standard reaction Gibbs energy, $Δ_{r} G^{0},$ of this reaction is positive. At the start of the reaction, there is one mole of $X_{2}$ and no X. As the reaction proceeds, the number of moles of X formed is given by $β$ . Thus, $β_{e q u i l i b r i u m}$ is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar $K^{- 1} m o l^{- 1}$ ).

The INCORRECT statement among the following, for this reaction is:

Decrease in the total pressure will result in formation of more moles of gaseous X

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At the start of the reaction, dissociation of gaseous

X_{2}

takes place spontaneously

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β_{e q u i l i b r i u m} = 0.7

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K_{c} < 1

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Solution

The correct option is C $β_{e q u i l i b r i u m} = 0.7$
There is no data given to find the $β_{e q u i l i b r i u m}$ exact value.
$Δ G_{c}^{0} = - 2.303 R T l o g K_{c}$
$l o g K_{c} = - 1$
$K_{c} < 1$

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Similar questions

Q. Thermal decomposition of gaseous

X_{2}

to gaseous X at 298 K takes place according to the following equation:

X_{2} (g) ⇌ 2 X (g)

The standard reaction Gibbs energy,

Δ_{r} G^{0},

of this reaction is positive. At the start of the reaction, there is one mole of

X_{2}

and no X. As the reaction proceeds, the number of moles of X formed is given by

β

. Thus,

β_{e q u i l i b r i u m}

is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar

K^{- 1} m o l^{- 1}

).

The INCORRECT statement among the following, for this reaction is:

Q. Thermal decomposition of gaseous

X_{2}

to gaseous X at 298 K takes place according to the following equation:

X_{2} (g) ⇌ 2 X (g)

The standard reaction Gibbs energy,

Δ_{r} G^{0},

of this reaction is positive. At the start of the reaction, there is one mole of

X_{2}

and no X. As the reaction proceeds, the number of moles of X formed is given by

β

. Thus,

β_{e q u i l i b r i u m}

is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar

K^{- 1} m o l^{- 1}

)

The equilibrium constant

K_{p}

for this reaction at 298 K, in terms of

β_{e q u i l i b r i u m},

is:

Q. Thermal decomposition of gaseous

X_{2}

to gaseous X at 298 K takes place according to the following equation:

X_{2} (g) ⇌ 2 X (g)

The standard reaction Gibbs energy,

Δ_{r} G^{0},

of this reaction is positive. At the start of the reaction, there is one mole of

X_{2}

and no X. As the reaction proceeds, the number of moles of X formed is given by

β

. Thus,

β_{e q u i l i b r i u m}

is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given: R = 0.083 L bar

K^{- 1} m o l^{- 1}

).

The INCORRECT statement among the following, for this reaction is:

Q. The standard Gibbs energy change for a gaseous reaction at 27 is X Kcal. If equilibrium constant a reaction is 100 and R is 2 cal

K^{- 1} {m o l}^{- 1}

. Then X is:

C l_{2} (g) ⇌ 2 C l (g)

For the given reaction at equilibrium, moles of

C l_{2} (g)

is equal to the moles of Cl(g) and the equilibrium pressure is 1 atm. If

K_{p}

of this reaction is x

\times 10^{- 1}

, find x.

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The correct option is C βequilibrium=0.7There is no data given to find the βequilibrium exact value. ΔG0c=−2.303RT log Kc log Kc=−1 Kc<1

The correct option is C $β_{e q u i l i b r i u m} = 0.7$
There is no data given to find the $β_{e q u i l i b r i u m}$ exact value.
$Δ G_{c}^{0} = - 2.303 R T l o g K_{c}$
$l o g K_{c} = - 1$
$K_{c} < 1$