An indicator '$X$' is used for studying the effect of variation in concentration of iodide on the rate of reaction of iodide ion with $H_2O_2$ at room temperature. The indicator '$X$' forms a blue-colored complex with compound '$A$' present in the solution. The indicator '$X$' and compound '$A$' respectively are:
- AStarch and iodine
- BMethyl orange and $H_2O_2$
- CStarch and $H_2O_2$
- DMethyl orange and iodine
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Similar Questions
Consider a gas phase reaction which occurs in a closed vessel: $2 \ A \rightarrow 4 \ B + C$. The concentration of $B$ is found to be increased by $5 \times 10^{-3} \ mol \ L^{-1}$ in $10 \ s$. The rate of disappearance of $A$ (in $mol \ L^{-1} \ s^{-1}$) is:
In a hydrogenation reaction at $27\,^oC$,it is observed that the hydrogen gas pressure falls from $2\,atm$ to $1.2\,atm$ in $50\,min$. Calculate the rate of disappearance of hydrogen.
Medium
View SolutionFor the reaction $2N_2O_{5(g)} \to 4NO_{2(g)} + O_{2(g)}$,what is the ratio of the rate of decomposition of $N_2O_5$ to the rate of formation of $NO_2$?
Medium
View SolutionFor the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ under certain conditions of temperature and partial pressure of the reactants,the rate of formation of $NH_3$ is $0.001 \ kg \ L^{-1} \ h^{-1}$. The rate of consumption of $H_2$ under the same condition is $..... \ kg \ L^{-1} \ h^{-1}$.
Difficult
View SolutionIf the rate of reaction is given as $\frac{1}{3} \frac{d[X]}{dt} = -\frac{1}{2} \frac{d[Y]}{dt} = -\frac{d[Z]}{dt}$,the reaction can be represented as
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