A vessel of volume 24.6 L contains 1.5 moles of $\mathrm{H}_2$ and 2.5 moles of $\mathrm{N}_2$ at 300 K . Calculate the partial pressure of $\mathrm{N}_2$ in the vessel.
For a given unbalanced reaction, $\mathrm{MnO}_2+\mathrm{HCl} \longrightarrow \mathrm{MnCl}_2+\mathrm{H}_2 \mathrm{O}$, which is the limiting reagent, if the initial amount for each of the reactant is 100 grams?
[Molar masses : $\mathrm{MnO}_2=86.9 ; \mathrm{HCl}=36.5 ; \mathrm{MnCl}_2 \left.=125.8 ; \mathrm{Cl}_2=70.9 ; \mathrm{H}_2 \mathrm{O}=18\right]$
The emperical formula of a compound is $\mathrm{C}_2 \mathrm{H}_5 \mathrm{O}$ and its vapour density is 45 . What is the molecular formula of the compound?
Find the value of the equilibrium constant $(K)$ of a reaction at 300 K , when standard Gibbs free energy change is $-25 \mathrm{~kJ} \mathrm{~mol}^{-1}$ ? (Consider $R=8.33 \mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$ )
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