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 K⁻¹ mol⁻¹)
The equilibrium constant Kp for this reaction at 298 K, in terms of ???? ????????????????????????????????????????m, is
(A) 8????² ????????????????????????????????????????m / 2 - ???? ????????????????????????????????????????m (B) 8????² ????????????????????????????????????????m / 4 - ????² ????????????????????????????????????????m
(C) 4????² ????????????????????????????????????????m / 2 - ???? ????????????????????????????????????????m (D) 4????² ????????????????????????????????????????m / 4 - ????² ????????????????????????????????????????m
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