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3 years ago

2Al + 3CuSO4–>3Cu+ Al2(SO4)3

Chemistry

1 answer:

sergiy2304 [10]3 years ago

4 0

Answer:

7.82 g of Cu

Explanation:

2 moles of Al react to 3 moles of copper sulfate in order to produce 3 moles of copper and 1 mol of aluminum sulfate.

Firstly we determine the moles of reactant.

As copper sulfate is in excess, Al is the limiting.

2.75 g . 1mol /26.98g = 0.102 moles

Ratio is 2:3. 2 moles of Al, can produce 3 moles of Cu

So the 0.102 moles of Al will produce(0.102 . 3) /2 = 0.153 moles.

We convert moles to mass: 0.153 mol . 63.5g /mol = 9.71 g

That's the theoretical yield (100 % yield reaction)

We know that: (yield produced / theoretical yield) . 100 = percent yield

We replace:

(Yield produced / 9.71g) . 100 = 80.5 %

(Yield produced / 9.71g) = 0.805

Yield produced = 0.805 . 9.71g = 7.82 g

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4 years ago

Explain and illustrate the notation for distinguishing between the different p orbitals in a sublevel.

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Here, the three different notation of the p-orbital in different sub-level have to generate

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