At 273 K the maximum work done when pressure on 10 g of hydrogen is reduced from 10 atm to 1 atm under isothermal, reversible conditions is
(Assume the gas behaves ideally)
$$ \left(R=83 \mathrm{Jk}^{-1} \mathrm{~mol}^{-1}\right) $$
At $293 \mathrm{~K}, \Delta_r G^{\circ}$ for the following reaction is $165.469 \mathrm{~kJ} \mathrm{~mol}^{-1}$.
$$ \frac{3}{2} \mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{O}_3(\mathrm{~g}) $$
What is the equilibrium constant for this reaction?
$$ \left(R=83 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right) $$
At $T(\mathrm{~K})$, the solubility product of AgBr is $4 \times 10^{-13}$. What is its solubility in 0.1 M KBr solution?
The following equilibrium is established at STP.
$$ B_2(g) \rightleftharpoons 2 B(g) $$
Atoms of $B$ occupy $20 \%$ of total volume at STP. The total pressure of the system is 1 bar. What is its $K_p$ ? $($ STP volume $=22.7 \mathrm{~L})$
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