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Last updated date: 04th Dec 2023
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# The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 5}}M{s^{ - 1}}$. The rate of appearance of $S{O_3}$ is$A)0.64 \times {10^{ - 5}}M{s^{ - 1}} \\ B)0.32 \times {10^{ - 5}}M{s^{ - 1}} \\ C)2.56 \times {10^{ - 5}}M{s^{ - 1}} \\ D)1.28 \times {10^{ - 5}}M{s^{ - 1}} \\$

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Hint: For reactants the rate of disappearance is a positive number. For products the rate of disappearance is a negative number because they are being formed and not disappearing. For reactants the rate of formation is a negative number because they are disappearing and not being formed.

Reaction rate is calculated using the formula rate$= \dfrac{{\Delta [C]}}{{\Delta T}}$, where $\Delta [C]$ is the change in product concentration during time period $\Delta T$. The rate of reaction can be observed by watching the disappearance of a reactant or the appearance of a product over time.
Rate of disappearance is given as $- \dfrac{{\Delta [A]}}{{\Delta T}}$ where $A$ is a reactant. However, using this formula, the rate of disappearance cannot be negative. Also, if the negative rate of disappearance is essentially a positive rate of appearance.
So, for the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ the stoichiometric ratio of $S{O_2}$ and $S{O_3}$ are same. So the rate will be the same.
Therefore, the rate of disappearance of $S{O_2}$ and the rate of formation of $S{O_3}$ are the same.
So, the correct answer is $D)1.28 \times {10^{ - 5}}M{s^{ - 1}}$