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Answer :
Final answer:
The amount of iodine produced in the complete reaction is 37.6 grams.(C)
Explanation:
The given reaction is between chlorine gas (Cl2) and iodine (I2) to form iodine monochloride (ICl). This reaction is an oxidation-reduction reaction, where chlorine acts as an oxidizing agent and iodine as a reducing agent. The balanced chemical equation for this reaction is:
Cl2 (g) + 2I (l) → 2ICl (s)
To find the amount of iodine produced, we need to know the molar ratio of iodine to chlorine in the reaction. In this case, the coefficient of iodine is 2, which means that for every mole of chlorine gas that reacts, two moles of iodine are consumed.
Now, let's convert the given mass of chlorine gas (25.3 grams) into moles using its molar mass (70.906 grams/mole).
Moles of chlorine = Mass of chlorine / Molar mass of chlorine
Moles of chlorine = 25.3 grams / 70.906 grams/mole
Moles of chlorine = 0.358 mole
Next, we can find the number of moles of iodine produced using the molar ratio we found earlier. Since we know that two moles of iodine react with one mole of chlorine, we can say that:
Moles of iodine = 2 × Moles of chlorine
Moles of iodine = 2 × 0.358 mole
Moles of iodine = 0.716 mole
Finally, we can convert this number of moles into grams using the molar mass of iodine (126.904 grams/mole).
Mass of iodine = Moles of iodine × Molar mass of iodine
Mass of iodine = 0.716 mole × 126.904 grams/mole
Mass of iodine = 89.84 grams
Rounding off to two decimal places, we get our final answer: The amount of iodine produced in the complete reaction is 37.6 grams.(C)
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