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Question

Thermal decomposition of gaseous X2 to gaseous X at 298 K takes place according to the following equation:
X2(g)2X(g)
The standard reaction Gibbs energy, ΔrG0, of this reaction is positive. At the start of the reaction, there is one mole of X2 and no X. As the reaction proceeds, the number of moles of X formed is given by β. Thus, βequilibrium 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 K1mol1).

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

A
Decrease in the total pressure will result in formation of more moles of gaseous X
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B
At the start of the reaction, dissociation of gaseous X2 takes place spontaneously
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C
βequilibrium=0.7
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D
Kc<1
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Solution

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

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