The INCORRECT statement among the following, for this reaction, is | TestHub

Passage / Comprehension

Paragraph: 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, $Δ_{r} G^{\circ}$ , 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, $β_{equilibrium}$ 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 INCORRECT statement among the following, for this reaction, is

Options:

Answer:

Solution:

A] On decreasing $P_{T} [Q = \frac{n_{x^{2}} P_{T}}{n_{x_{2}} n_{T}}]$ Q will be less than $K_{p}$ reaction will move in forward direction
B] At the start of the reaction $∆ G = ∆ G^{o} + R T$ ln Q
$t = 0, Q = 0 \Rightarrow ∆_{r x n} G = - v e (s p o n t a n e o u s)$
C] If $β_{e q u i l i b r i u m} = 0.7$
$K_{p} = \frac{8 \times 0.49}{4 - 0.49} = \frac{3.92}{3.51}$
$K_{p} > 1$
Since it is given that
$∆ G^{o} > 0 \Rightarrow K_{p} < 1$
$∴$ This is incorrect
D] $K_{p} = K_{C} \times {(R T)}^{∆ n_{g}}$
$K_{C} = \frac{K_{p}}{{(R \times 298)}^{1}}$
$K_{C} < 1$

Chemistry - Thermodynamics - II Question with Solution | TestHub

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