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igomit [66]
3 years ago
6

How many atoms are in the 3.5 moles of arsenic atoms?

Chemistry
2 answers:
Elanso [62]3 years ago
7 0
2.1x10^24 I think maybe
Dmitry_Shevchenko [17]3 years ago
6 0
Number of atom in one mole = 6.022 × 10²³
So, in 3.5 moles, it would be: = 6.022 × 10²³ * 3.5 = 2.1 × 10²⁴

In short, Your Answer would be 2.1 × 10²⁴ atoms

Hope this helps!
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Answer:

1.5 moles of Fe produced.

Explanation:

Given data:

Moles of FeO react = 1.50 mol

Moles of iron produced = ?

Solution:

Chemical equation:

FeO + CO       →       Fe + CO₂

Now we will compare the moles of ironoxide with iron.

                           FeO          :           Fe

                              1             :             1

                             1.5           :           1.5

Thus from 1.5 moles of FeO 1.5 moles of Fe are produced.                                    

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What must two objects have in order for gravitational force to act on them speed gorse mass orbit
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Alum is a compound used in a variety of applications including cosmetics, water purification, and as a food additive. It can be
vlabodo [156]

Answer:

The theoretical yield of alum is 19.873 grams and percent yield for this alum synthesis is 45.33%.

Explanation:

Mass of bottle = 10.221 g

Mass of bottle with aluminium pieces = 11.353 g

Mass of aluminium = 11.353 g - 10.221 g = 1.132 g

Mass of alum and bottle = 19.230 g

Mass of alum =  19.230 g - 10.221 g = 9.009 g

Experimental yield of alum =  9.009 g

Theoretical yield of alum:

2Al(s) +2 KOH(aq) +4H_2SO_4(aq)+10 H_2O(l) \rightarrow 2 KAl(SO_4)_2.12 H_2O(s)+3H_2(g)

Moles of aluminium = \frac{1.132 g}{27 g/mol}=0.041926 mol

According to reaction, 2 moles of aluminum gives 2 moles of alum.

Then 0.041926 mol aluminium will give :

\frac{2}{2}\times 0.041926 mol=0.041926 mol of alum.

Mass of 0.041926 moles of alum:

0.041926 mol × 474 g/mol= 19.873 g

Theoretical yield of alum = 19.873 g

Percentage yield:

\% Yield =\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Percentage yield of the alum:

\% Yield =\frac{ 9.009 g}{19.873 g}\times 100=45.33\%

The theoretical yield of alum is 19.873 grams and percent yield for this alum synthesis is 45.33%.

7 0
3 years ago
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