The isobars of one mole of an ideal gas were obtained at three different pressure ( $p_1, p_2$ and $p_3$ ). The slopes of these isobars are $m_1, m_2$ and $m_3$ respectively. If $p_1 < p_2 < p_3$, then the correct relation of the slopes is
100 mL of $0.05 \mathrm{M} \mathrm{Cu}^{2+}$ aqueous solution is added to IL of 0.1 M KI solution. The number of moles of $\mathrm{I}_2$ and $\mathrm{Cu}_2 \mathrm{I}_2$ formed are respectively.
The $C_p$ of an ideal gas is $10314 \mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$. One mole of this gas is expanded against a constant pressure of $p \mathrm{~atm}$. The change in temperature during expansion is 1.0 K . The value of $q$ (in J ) and $\Delta H$ (in $\mathrm{Jmol}^{-1}$ ) are respectively.
At $T(\mathrm{~K}), K_p$ value for the reaction,
$$ 2 \mathrm{AO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{AO}_3(\mathrm{~g}) \text { is } 4 \times 10^{10}, $$
What is the $K_p^{\prime}$ value for
$$ 2 \mathrm{AO}_2(\mathrm{~g})+\frac{3}{2} \mathrm{O}_2 \rightleftharpoons 3 \mathrm{AO}_3(\mathrm{~g}) \text { at } T(\mathrm{~K}) $$
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