320197 The rate law equation for a reaction between \(\mathrm{A}, \mathrm{B}\) and \(\mathrm{C}\) is \(\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}][\mathrm{C}]^{2}\), what will be new rate of reaction if concentration of both \(\mathrm{A}\) and \(\mathrm{B}\) are doubled.

320198 The rate of reaction between \(\mathrm{BrO}_{3}^{-}\)and \(\mathrm{Br}^{-}\)is given by the rate law:
\(\frac{{{\rm{d}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]}}{{{\rm{dt}}}}{\rm{ = k}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]\left[ {{\rm{B}}{{\rm{r}}^{\rm{ - }}}} \right]{\left[ {{{\rm{H}}^{\rm{ + }}}} \right]^{\rm{2}}}\)
This indicates :

320199 According to law of mass action, rate of a chemical reaction is proportional to

320200 For the process \(2 \mathrm{~A} \rightarrow\) products, rate of reaction w.r.t \({\text{A}}\) at 10 seconds is \(2 \times 10^{-2} \mathrm{Ms}^{-1}\) then rates of same process at 5 and 15 seconds \(\quad(\) order \(\neq 0\) ) respectively are (in \(\mathrm{M} / \mathrm{s}\) )

320197 The rate law equation for a reaction between \(\mathrm{A}, \mathrm{B}\) and \(\mathrm{C}\) is \(\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}][\mathrm{C}]^{2}\), what will be new rate of reaction if concentration of both \(\mathrm{A}\) and \(\mathrm{B}\) are doubled.

320198 The rate of reaction between \(\mathrm{BrO}_{3}^{-}\)and \(\mathrm{Br}^{-}\)is given by the rate law:
\(\frac{{{\rm{d}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]}}{{{\rm{dt}}}}{\rm{ = k}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]\left[ {{\rm{B}}{{\rm{r}}^{\rm{ - }}}} \right]{\left[ {{{\rm{H}}^{\rm{ + }}}} \right]^{\rm{2}}}\)
This indicates :

320199 According to law of mass action, rate of a chemical reaction is proportional to

320200 For the process \(2 \mathrm{~A} \rightarrow\) products, rate of reaction w.r.t \({\text{A}}\) at 10 seconds is \(2 \times 10^{-2} \mathrm{Ms}^{-1}\) then rates of same process at 5 and 15 seconds \(\quad(\) order \(\neq 0\) ) respectively are (in \(\mathrm{M} / \mathrm{s}\) )

320197 The rate law equation for a reaction between \(\mathrm{A}, \mathrm{B}\) and \(\mathrm{C}\) is \(\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}][\mathrm{C}]^{2}\), what will be new rate of reaction if concentration of both \(\mathrm{A}\) and \(\mathrm{B}\) are doubled.

320198 The rate of reaction between \(\mathrm{BrO}_{3}^{-}\)and \(\mathrm{Br}^{-}\)is given by the rate law:
\(\frac{{{\rm{d}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]}}{{{\rm{dt}}}}{\rm{ = k}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]\left[ {{\rm{B}}{{\rm{r}}^{\rm{ - }}}} \right]{\left[ {{{\rm{H}}^{\rm{ + }}}} \right]^{\rm{2}}}\)
This indicates :

320199 According to law of mass action, rate of a chemical reaction is proportional to

320200 For the process \(2 \mathrm{~A} \rightarrow\) products, rate of reaction w.r.t \({\text{A}}\) at 10 seconds is \(2 \times 10^{-2} \mathrm{Ms}^{-1}\) then rates of same process at 5 and 15 seconds \(\quad(\) order \(\neq 0\) ) respectively are (in \(\mathrm{M} / \mathrm{s}\) )

320197 The rate law equation for a reaction between \(\mathrm{A}, \mathrm{B}\) and \(\mathrm{C}\) is \(\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}][\mathrm{C}]^{2}\), what will be new rate of reaction if concentration of both \(\mathrm{A}\) and \(\mathrm{B}\) are doubled.

320198 The rate of reaction between \(\mathrm{BrO}_{3}^{-}\)and \(\mathrm{Br}^{-}\)is given by the rate law:
\(\frac{{{\rm{d}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]}}{{{\rm{dt}}}}{\rm{ = k}}\left[ {{\rm{BrO}}_{\rm{3}}^{\rm{ - }}} \right]\left[ {{\rm{B}}{{\rm{r}}^{\rm{ - }}}} \right]{\left[ {{{\rm{H}}^{\rm{ + }}}} \right]^{\rm{2}}}\)
This indicates :

320199 According to law of mass action, rate of a chemical reaction is proportional to

320200 For the process \(2 \mathrm{~A} \rightarrow\) products, rate of reaction w.r.t \({\text{A}}\) at 10 seconds is \(2 \times 10^{-2} \mathrm{Ms}^{-1}\) then rates of same process at 5 and 15 seconds \(\quad(\) order \(\neq 0\) ) respectively are (in \(\mathrm{M} / \mathrm{s}\) )