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
For a reaction,$2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$. The $N_2O_5$ disappears at a rate of $0.06 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of $NO_{2(g)}$ formation (in $mol \ dm^{-3} \ s^{-1}$)?
The differential rate law for the reaction $H_2 + I_2 \to 2HI$ is
MediumAIEEE 2002
View SolutionFor a reaction,$2A + B \rightarrow 2C$,the rate of disappearance of $A$ is $0.076 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of disappearance of $B$?
In the reaction $xA \to yB,$
$0.48 + \log \left\{ -\frac{d[A]}{dt} \right\} = \log \left\{ +\frac{d[B]}{dt} \right\} + 0.7$
Then,$x : y$ is
$0.48 + \log \left\{ -\frac{d[A]}{dt} \right\} = \log \left\{ +\frac{d[B]}{dt} \right\} + 0.7$
Then,$x : y$ is
Difficult
View SolutionConsider the following reaction: $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$. The rate of this reaction in terms of $N_2$ at $T \ K$ is $\frac{-d[N_2]}{dt} = 0.02 \ mol \ L^{-1} \ s^{-1}$. What is the value of $\frac{-d[H_2]}{dt}$ (in units of $mol \ L^{-1} \ s^{-1}$) at the same temperature?
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