First slide

Chemical Equilibrium

Question

Which are true for the reaction : $A_{2} ⇌ 2 C + D ?$

Moderate

A

if $∆ H = 0; K_{p}$ and $α$ (alpha) increases with increase in temperature
B

if $∆ H = + ve, K_{p}$ increases with temperature and dissociation of A₂ increases.
C

if $∆ H = - ve, K_{p}$ decreases with temperature and dissociation of A₂ decreases.
D

$K_{p} = 4 α^{3} {[\frac{P}{1 + 2 α}]}^{2}$

Solution

$A ⇌ 2 C + D Initial 1 0 0 At equilibrium 1 - α 2 α α K_{p} = {(2 α)}^{2} α \times {[\frac{P}{∆ n}]}^{2} = \frac{4 α^{3} P^{2}}{{(1 + 2 α)}^{2}} Use 2.303 \log \frac{K_{2}}{K_{1}} = \frac{∆ H}{R} [\frac{T_{2} - T_{1}}{T_{1} T_{2}}] for effect of temperature on K .$

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