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Calculate the maximum numbers of moles and grams of iodic
Chapter 3, Problem 50P(choose chapter or problem)
Calculate the maximum numbers of moles and grams of iodic acid (\(\mathrm{HIO}_{3}\)) that can form when \(635 g\) of iodine trichloride reacts with \(118.5 g\) of water:
\(\mathrm{ICl}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{ICl}+\mathrm{HIO}_{3}+\mathrm{HCl}\) [unbalanced]
What mass of the excess reactant remains?
Questions & Answers
QUESTION:
Calculate the maximum numbers of moles and grams of iodic acid (\(\mathrm{HIO}_{3}\)) that can form when \(635 g\) of iodine trichloride reacts with \(118.5 g\) of water:
\(\mathrm{ICl}_{3}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{ICl}+\mathrm{HIO}_{3}+\mathrm{HCl}\) [unbalanced]
What mass of the excess reactant remains?
ANSWER:Step 1 of 4
Here we have to calculate the maximum numbers of moles and grams of iodic acid () that can form when 635 g of iodine trichloride reacts with 118.5 g of water and have to find out the mass of the excess reactant remains present in the reaction.
The given unbalanced chemical equation is,
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