A solid mixture weighing 5 g contains equal number of moles of $\mathrm{Na}_2 \mathrm{CO}_3$ and NaHCO . This solid mixture was dissolved in 1 L of water. What is the volume (in mL ) of 0.1 M HCl required to completely react with this 1 L mixture solution?
At 298 K the equilibrium constant for the reaction $M(s)+2 \mathrm{Ag}^{+}(a q) \longrightarrow M^{2+}(a q)+2 \mathrm{Ag}(s)$ is $10^{15}$. What is the $E_{\text {cell }}^{\ominus}$ (in V) for this reaction?
$$ \left(\frac{2.303 R T}{F}\right)=0.06 \mathrm{~V} $$
$A \rightarrow P$ is a first order reaction. At 300 K this reaction was started with $[A]=0.5 \mathrm{~mol} \mathrm{~L}^{-1}$.
The rate constant of reaction was $0.125 \mathrm{~min}^{-1}$. The same reaction was started separately with $[A]=1 \mathrm{molL}^{-1}$ at 300 K . The rate constant (in $\mathrm{min}^{-1}$ ) now is
Observe the following reaction
I. $\mathrm{CO}(\mathrm{g})+\mathrm{H}_2(\mathrm{~g}) \xrightarrow{X} \mathrm{HCHO}(\mathrm{g})$
II. $\mathrm{CO}(\mathrm{g})+3 \mathrm{H}_2(\mathrm{~g}) \xrightarrow{\gamma} \mathrm{CH}_4(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\mathrm{g})$
The catalysts $X$ and $Y$ in the above reactions are respectively
TS EAMCET Papers
All year-wise previous year question papers