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What are 25.4 g of iodine and 14.2 g of cl made to react completely to yield a mixture of icl and icl3 cal the no of moles of icl and icl3?
Wiki User
∙ 11y ago
I2 + 2Cl2 .==> ICl + ICl3
molar mass of I2 = 127
molar mass of Cl2 = 70.9
moles of I2 used = 25.4/127 = 0.2 moles of I2
moles of Cl2 used = 14.2/70.9 = 0.2 moles of Cl2
Since the stoichiometry indicates that each mole of I2 reacts with 2 moles of Cl2 to give 1 mole each of ICl and ICl3, you should get 0.1 moles of each product. The reason you don't get 0.2 moles is because the amount of I2 is limiting, and you can see that 2 moles of Cl2 will use up 1 mole of I2, so 0.2 moles of Cl2 will use up 0.1 moles of I2. So 0.1 moles of product is all you can get under these conditions
Wiki User
∙ 11y ago
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