Identify the conditions at which van der Waals' equation of state changes to ideal gas equation.
Observe the following
I. 0.0063
II. 132.00
III. 1004
The number of significant figures in I, II and III is respectively.
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?
$$ \left(R=83 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right) $$
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