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Ivan
2 years ago
7

Aqueous Copper (II) nitrate reacts with aqueous potassium iodide to form Copper (II) iodide solid and potassium nitrate

Chemistry
1 answer:
nikitadnepr [17]2 years ago
7 0

Answer:

Cu(NO₃)₂ (aq) + 2 KI (aq) ---> CuI₂ (s) + 2 KNO₃

Explanation:

When writing the reaction with the symbols, you need to take into account the charges of the ions. If he charges on the ions do not balance out in a molecule, they need to be made up for in the form of subscripts. For example, copper (+2) and iodine (-1) have charges which do not balance. Thus, to make the molecule neutral, you need to have two iodine atoms (CuI₂).

The unbalanced equation:

Cu(NO₃)₂ (aq) + KI (aq) ---> CuI₂ (s) + KNO₃

<u>Reactants</u>: 1 copper, 2 nitrate, 1 potassium, 1 iodine

<u>Products</u>: 1 copper, 1 nitrate, 1 potassium, 2 iodine

The balanced equation:

1 Cu(NO₃)₂ (aq) + 2 KI (aq) ---> 1 CuI₂ (s) + 2 KNO₃

<u>Reactants</u>: 1 copper, 2 nitrate, 2 potassium, 2 iodine

<u>Products</u>: 1 copper, 2 nitrate, 2 potassium, 2 iodine

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Answer:

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Explanation:

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Recall that water's molecular formula is H₂O. It contains hydrogen and oxygen. Look up the two elements masses on the Periodic Table.

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Use the molar mass as a ratio.

\frac{18.015 \ g \ H_2 O}{ 1 \ mol \ H_2 O}

Multiply by the given number of moles.

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The moles of water will cancel.

3 *\frac{18.015 \ g \ H_2 O}{ 1 }

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