Question

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$\rm\small\fbox\red{Question:-}$

=>2 moles of zinc reacts with a cupric
$\rm \: solution \: containing \: 6.023 \times {10}^{22}$

$\rm \: formula \: of \: cucl_{2}.$
Calculate the mole of copper obtained.


$\rm \red {z_{(s)} + cucl_{2} \rightarrow zncl_{(aq)} + cu_{(s)}}$
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Answer 1

Answer:

First write down the equation that takes place:

Zn + CuCl2 ----------> ZnCl2 + Cu

There 1 mole of Zn will react with 1 mole of CuCl2 to give 1 mole of Cu.

From the question we have 2 moles of zinc, and

CuCl2 has 6.023x10^22 formula units(calculate its moles)

If 6.023x10^23 (avagadro's constant) = 1 mole

then, 6.023x10^22 = 1 mole x 6.023 x10^22/6.023x10^23

= 1 mole x 10^22/10^23

= 1 mole x 10^-1

= 0.1 moles

Find the limiting factor as not all the Zinc will react with the cupric chloride:

Since 1 mole of zinc requires 1 mole of CuCl2 to give 1 mole of copper, while in this case there is only 0.1 moles of CuCl2, then CuCl2 is the limiting factor and is what we use for the calculation as follows:

If 1 mole of CuCl2 gives 1 mole of Cu.

Then how much will 0.1 mole of CuCl2 give = 1mole x 0.1 mole/1mole

= 0.1 moles

Therefore moles of Cu obtained is 0.1 moles

Explanation:

Hope it will help you..