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algol [13]
3 years ago
12

How many atoms are in Cu2MgHO

Chemistry
1 answer:
Illusion [34]3 years ago
4 0
To find how many atoms are in the compound, we first have to find how many moles there are. The numbers in the subscript tell you how many moles of each element are present in the compound. Therefore, to find the number of total moles, we can add up each of the numbers in the subscript:

Cu₂Mg₁H₁O₁  *when there is no number under an element, it is implied that there is 1 mole of the element
2+1+1+1=5 moles

We can then use Avogadro's number and dimensional analysis to find how many atoms are in the compound (Avogadro's number is 6.02x10^23):

5 moles (6.02x10^23/1 mole)= 3.01x10^24 atoms
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4 0
1 year ago
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Hunter-Best [27]

Answer:

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5 0
3 years ago
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In reality, a hydrate of iron(III) nitrate had to be used, not the anhydrous salt. As you may guess, some of the hydrate’s mass
liq [111]

<u>Answer:</u> The mass of nonahydrate iron (III) nitrate is 16.2 g

<u>Explanation:</u>

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

Molarity of Fe(NO_3)_3 = 0.0020 M

Volume of solution = 2 L

Putting values in above equation, we get:

0.0200M=\frac{\text{Moles of }Fe(NO_3)_3}{2L}\\\\\text{Moles of }Fe(NO_3)_3=(0.0200mol/L\times 2L)=0.04mol

The chemical equation for the decomposition of hydrated iron (III) nitrate follows:

Fe(NO_3)_3.9H_2O\rightarrow Fe(NO_3)_3+9H_2O

By Stoichiometry of the reaction:

1 mole of iron (III) nitrate is produced from 1 mole of hydrated iron (III) nitrate

So, 0.04 moles of iron (III) nitrate will be produced from = \frac{1}{1}\times 0.04=0.04mol of hydrated iron (III) nitrate

To calculate the mass from given number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Molar mass of nonahydrate iron (III) nitrate = 404.0 g/mol

Moles of nonahydrate iron (III) nitrate = 0.04 moles

Putting values in above equation, we get:

0.04mol=\frac{\text{Mass of nonahydrate iron (III) nitrate}}{404.0g/mol}\\\\\text{Mass of nonahydrate iron (III) nitrate}=(0.04mol\times 404.0g/mol)=16.2g

Hence, the mass of nonahydrate iron (III) nitrate is 16.2 g

7 0
3 years ago
Why is a measured amount of water needed to determine the specific heat of a metal object?
shutvik [7]
This  is  because  absorbed  heat  energy or  released  by  water  is dependent on  mass of  water.
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where  q is  the amount  of  energy  required,   m  is  the  mass , C  is   the  specific  heat  capacity  and  delta  T is change  in  temperature.
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