Question

The molar mass of copper(II) chloride (CuCl2) is 134. 45 g/mol. How many formula units of CuCl2 are present in 17. 6 g of CuCl2? 7. 88 × 1022 formula units 1. 84 × 1023 formula units 1. 91 × 1023 formula units 1. 42 × 1024 formula units.

Answer 1

The number of formula units in the 17.6 g copper (II) chloride sample is $7.88\;\times\;10^2^2$option A is correct.

The formula unit is given as the molecule of the compound with constituent atoms and bonds.

Computation for the number of formula units

The number of formula units in a mole of sample is equal to the Avogadro number. The Avogadro number is a constant with the value of $6.023\;\times\;10^2^3$.

Thus, the number of formula units in copper (II) chloride are:

$\rm 1\;mol=6.023\;\times\;10^2^3\;formula\;unit\\134.45\;g/mol=6.023\;\times\;10^2^3\;formula\;unit$

The given mass of copper chloride is 17.6 g. The number of formula units is given as:

$\rm 134.45\;g=6.023\;\times\;10^2^3\;units\\\\17.6\;g=\dfrac{6.023\;\times\;10^2^3}{134.45}\;\times\;17.6\;units\\\\ 17.6\;g=7.88\;\times\;10^2^2\;units$

The number of formula units in the 17.6 g copper (II) chloride sample is $7.88\;\times\;10^2^2$ units.

Thus, option A is correct.

Learn more about formula units, here:

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