Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation:
2ClO2(aq) + 2OH–(aq) —> ClO2–(aq) + ClO3–(aq) + H2O(l)
Under a certain set of conditions, the initial rate of disappearance of chlorine dioxide was determined to be 2.30 x 10–1 M/s. What is the initial rate of appearance of chlorite ion under those same conditions?
1/2delta(ClO2)/dt = d(ClO2-)/dt
If rate for Cl2O is 0.230 then divide by 2 to find the rate of ClO2^-.
In kinetics. the equation tells you that the rate of Cl2O is twice as fast as ClO2^-
To determine the initial rate of appearance of chlorite ion (ClO2–), we need to examine the stoichiometry of the balanced chemical equation.
According to the equation:
2ClO2(aq) + 2OH–(aq) —> ClO2–(aq) + ClO3–(aq) + H2O(l)
We can see that for every 2 moles of ClO2 that disappear, 1 mole of ClO2– appears. Therefore, the initial rate of appearance of ClO2– is given by half of the initial rate of disappearance of ClO2.
Given that the initial rate of disappearance of ClO2 is 2.30 x 10–1 M/s, the initial rate of appearance of ClO2– would be half of that:
Initial rate of appearance of ClO2– = 1/2 * initial rate of disappearance of ClO2
Initial rate of appearance of ClO2– = 1/2 * 2.30 x 10–1 M/s
Initial rate of appearance of ClO2– = 1.15 x 10–1 M/s
Therefore, the initial rate of appearance of chlorite ion under those same conditions is 1.15 x 10–1 M/s.
To find the initial rate of appearance of the chlorite ion (ClO2-), we need to determine its stoichiometric coefficient in the balanced chemical equation.
By looking at the equation, we can see that two chlorine dioxide molecules (ClO2) react to form one chlorite ion (ClO2-).
Since the stoichiometric coefficient of chlorite ion is 1, the initial rate of appearance of chlorite ion will also be 2.30 x 10–1 M/s.
Therefore, the initial rate of appearance of chlorite ion under those same conditions is 2.30 x 10–1 M/s.