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

Reactants: 1 copper, 2 nitrate, 1 potassium, 1 iodine

Products: 1 copper, 1 nitrate, 1 potassium, 2 iodine

The balanced equation:

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

Reactants: 1 copper, 2 nitrate, 2 potassium, 2 iodine

Products: 1 copper, 2 nitrate, 2 potassium, 2 iodine

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Thomas had a volume of 8.5 g of sodium chloride. What is the molar mass.?

alina1380 [7]

Answer:

58.44 g/mol

Explanation:

In this problem, make sure to remember that volume is measured in mL, L or any other units of volume. Remember that g represents grams, and grams is a measure of mass.

However, independent of what mass or what volume we take, molar mass is known to be an intensive property. That is, molar mass doesn't depend on any external conditions or any measurements.

Molar mass solely depends on the chemical structure of a compound and is a constant number at any given conditions.

In this problem, we are given sodium chloride, NaCl. In order to find its molar mass, we need to refer to the periodic table, find the atomic masses of Na and Cl and then add them up to have the molar mass of NaCl:

$M_{NaCl} = M_{Na} + M_{Cl} = 22.99 g/mol + 35.453 g/mol = 58.44 g/mol$