How much I2 is needed to stop decomposition of H2O2?
To determine how much I2 is needed to stop the decomposition of H2O2, we can use the balanced chemical equation for the reaction between I2 and H2O2. The reaction can be represented as follows:
2 H2O2(aq) + 2 I2(aq) → 2 H2O(l) + 2 HI(aq) + O2(g)
From the equation, you can see that 2 moles of iodine (I2) are required to react with 2 moles of hydrogen peroxide (H2O2). Therefore, the molar ratio of I2 to H2O2 is 1:1.
To determine the amount of I2 needed to stop the decomposition of H2O2, you need to know the amount of H2O2 present. Let's assume you have a certain volume of H2O2 solution and its concentration is given in moles per liter (M).
1. First, convert the volume of H2O2 solution to moles using its concentration (Molarity = moles of solute / liters of solution):
moles of H2O2 = concentration (M) × volume (L)
2. Since the molar ratio of I2 to H2O2 is 1:1, the number of moles of I2 required will be the same as the moles of H2O2:
moles of I2 required = moles of H2O2
Once you have determined the moles of I2 required, you can convert it to grams if needed by using the molar mass of iodine (I2), which is approximately 253.8 g/mol:
grams of I2 required = moles of I2 × molar mass of I2
By following these steps, you can calculate the amount of I2 needed to stop the decomposition of H2O2 based on the concentration and volume of the H2O2 solution.