320306
Assertion :
The decomposition of gaseous \(\mathrm{N}_{2} \mathrm{O}_{5}\) follows first order kinetics.
Reason :
The plot of log of its partial pressure versus time is linear with slope, \({\rm{ - }}\frac{{\rm{k}}}{{{\rm{2}}{\rm{.303}}}}\) and having intercept equal to \(\log \mathrm{P}\).
320307 \(\mathrm{A} \rightarrow \mathrm{B}\) is a first order reaction. The initial concentration of \({\text{A}}\) is \(0.2 \mathrm{~mol} \mathrm{~L}^{-1}\). After \(10 \mathrm{~min}\), the concentration of \({\text{B}}\) is found to be \(0.18 \mathrm{~mol}\) \(\mathrm{L}^{-1}\). The rate constant (in \(\min ^{-1}\) ) for the reaction is:
320308
Acid hydrolysis of ester is first order reaction and rate constant is given by
\({\text{k}} = \frac{{2.303}}{{\text{t}}}\,\,{\text{log}}\,\,\frac{{{{\text{V}}_\infty } - {{\text{V}}_0}}}{{{{\text{V}}_\infty } - {{\text{V}}_{\text{t}}}}}\)
where, \({{\text{V}}_0},{{\text{V}}_t}\) and \({{\text{V}}_\infty }\) are the volumes of standard \(\mathrm{NaOH}\) required to neutralise acid present at a given time, if ester is \(50 \%\) neutralised then
320306
Assertion :
The decomposition of gaseous \(\mathrm{N}_{2} \mathrm{O}_{5}\) follows first order kinetics.
Reason :
The plot of log of its partial pressure versus time is linear with slope, \({\rm{ - }}\frac{{\rm{k}}}{{{\rm{2}}{\rm{.303}}}}\) and having intercept equal to \(\log \mathrm{P}\).
320307 \(\mathrm{A} \rightarrow \mathrm{B}\) is a first order reaction. The initial concentration of \({\text{A}}\) is \(0.2 \mathrm{~mol} \mathrm{~L}^{-1}\). After \(10 \mathrm{~min}\), the concentration of \({\text{B}}\) is found to be \(0.18 \mathrm{~mol}\) \(\mathrm{L}^{-1}\). The rate constant (in \(\min ^{-1}\) ) for the reaction is:
320308
Acid hydrolysis of ester is first order reaction and rate constant is given by
\({\text{k}} = \frac{{2.303}}{{\text{t}}}\,\,{\text{log}}\,\,\frac{{{{\text{V}}_\infty } - {{\text{V}}_0}}}{{{{\text{V}}_\infty } - {{\text{V}}_{\text{t}}}}}\)
where, \({{\text{V}}_0},{{\text{V}}_t}\) and \({{\text{V}}_\infty }\) are the volumes of standard \(\mathrm{NaOH}\) required to neutralise acid present at a given time, if ester is \(50 \%\) neutralised then
320306
Assertion :
The decomposition of gaseous \(\mathrm{N}_{2} \mathrm{O}_{5}\) follows first order kinetics.
Reason :
The plot of log of its partial pressure versus time is linear with slope, \({\rm{ - }}\frac{{\rm{k}}}{{{\rm{2}}{\rm{.303}}}}\) and having intercept equal to \(\log \mathrm{P}\).
320307 \(\mathrm{A} \rightarrow \mathrm{B}\) is a first order reaction. The initial concentration of \({\text{A}}\) is \(0.2 \mathrm{~mol} \mathrm{~L}^{-1}\). After \(10 \mathrm{~min}\), the concentration of \({\text{B}}\) is found to be \(0.18 \mathrm{~mol}\) \(\mathrm{L}^{-1}\). The rate constant (in \(\min ^{-1}\) ) for the reaction is:
320308
Acid hydrolysis of ester is first order reaction and rate constant is given by
\({\text{k}} = \frac{{2.303}}{{\text{t}}}\,\,{\text{log}}\,\,\frac{{{{\text{V}}_\infty } - {{\text{V}}_0}}}{{{{\text{V}}_\infty } - {{\text{V}}_{\text{t}}}}}\)
where, \({{\text{V}}_0},{{\text{V}}_t}\) and \({{\text{V}}_\infty }\) are the volumes of standard \(\mathrm{NaOH}\) required to neutralise acid present at a given time, if ester is \(50 \%\) neutralised then
320306
Assertion :
The decomposition of gaseous \(\mathrm{N}_{2} \mathrm{O}_{5}\) follows first order kinetics.
Reason :
The plot of log of its partial pressure versus time is linear with slope, \({\rm{ - }}\frac{{\rm{k}}}{{{\rm{2}}{\rm{.303}}}}\) and having intercept equal to \(\log \mathrm{P}\).
320307 \(\mathrm{A} \rightarrow \mathrm{B}\) is a first order reaction. The initial concentration of \({\text{A}}\) is \(0.2 \mathrm{~mol} \mathrm{~L}^{-1}\). After \(10 \mathrm{~min}\), the concentration of \({\text{B}}\) is found to be \(0.18 \mathrm{~mol}\) \(\mathrm{L}^{-1}\). The rate constant (in \(\min ^{-1}\) ) for the reaction is:
320308
Acid hydrolysis of ester is first order reaction and rate constant is given by
\({\text{k}} = \frac{{2.303}}{{\text{t}}}\,\,{\text{log}}\,\,\frac{{{{\text{V}}_\infty } - {{\text{V}}_0}}}{{{{\text{V}}_\infty } - {{\text{V}}_{\text{t}}}}}\)
where, \({{\text{V}}_0},{{\text{V}}_t}\) and \({{\text{V}}_\infty }\) are the volumes of standard \(\mathrm{NaOH}\) required to neutralise acid present at a given time, if ester is \(50 \%\) neutralised then
320306
Assertion :
The decomposition of gaseous \(\mathrm{N}_{2} \mathrm{O}_{5}\) follows first order kinetics.
Reason :
The plot of log of its partial pressure versus time is linear with slope, \({\rm{ - }}\frac{{\rm{k}}}{{{\rm{2}}{\rm{.303}}}}\) and having intercept equal to \(\log \mathrm{P}\).
320307 \(\mathrm{A} \rightarrow \mathrm{B}\) is a first order reaction. The initial concentration of \({\text{A}}\) is \(0.2 \mathrm{~mol} \mathrm{~L}^{-1}\). After \(10 \mathrm{~min}\), the concentration of \({\text{B}}\) is found to be \(0.18 \mathrm{~mol}\) \(\mathrm{L}^{-1}\). The rate constant (in \(\min ^{-1}\) ) for the reaction is:
320308
Acid hydrolysis of ester is first order reaction and rate constant is given by
\({\text{k}} = \frac{{2.303}}{{\text{t}}}\,\,{\text{log}}\,\,\frac{{{{\text{V}}_\infty } - {{\text{V}}_0}}}{{{{\text{V}}_\infty } - {{\text{V}}_{\text{t}}}}}\)
where, \({{\text{V}}_0},{{\text{V}}_t}\) and \({{\text{V}}_\infty }\) are the volumes of standard \(\mathrm{NaOH}\) required to neutralise acid present at a given time, if ester is \(50 \%\) neutralised then