Tin has ten stable isotopes. The heaviest, 124Sn, makes up 5.80% of naturally occuring tin atoms. How many atoms of 124Sn are pr
1 answer:
The average atomic mass of Sn is 118.71 g/mol
the percentage of heaviest Sn is 5.80%
the given mass of Sn is 82g
The total moles of Sn will be = mass / atomic mass = 82/118.71=0.691
Total atoms of Sn in 82g =
the percentage of heaviest Sn is 5.80%
So the total atoms of = 5.80% X
Total atoms of =
atoms
the mass of will be =
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Answer:
The partial pressure of carbon dioxide is 22.8 mmHg
Explanation:
Dalton's Law is a gas law that relates the partial pressures of the gases in a mixture. This law says that the pressure of a gas mixture is equal to the sum of the partial pressures of all the gases present.
In this case:
Ptotal=Pnitrogen + Poxygen + Pcarbondioxide
You know that:
- Ptotal= 0.998 atm
- Pnitrogen= 0.770 atm
- Poxygen= 0.198 atm
- Pcarbondioxide= ?
Replacing:
0.998 atm=0.770 atm + 0.198 atm + Pcarbondioxide
Solving:
Pcarbondioxide= 0.998 atm - 0.770 atm - 0.198 atm
Pcarbondioxide= 0.03 atm
Now you apply the following rule of three: if 1 atm equals 760 mmHg, 0.03 atm how many mmHg equals?
Pcarbondioxide= 22.8 mmHg
<u><em>The partial pressure of carbon dioxide is 22.8 mmHg</em></u>
Answer:
1.82 g is the maximum mass of CuS.
Explanation:
Considering:
Or,
Given :
<u>For :
</u>
Molarity = 0.500 M
Volume = 38.0 mL
The conversion of mL to L is shown below:
1 mL = 10⁻³ L
Thus, volume = 38.0×10⁻³ L
Thus, moles of :
<u>Moles of = 0.019 moles
</u>
<u>For :
</u>
Molarity = 0.600 M
Volume = 42.0 mL
The conversion of mL to L is shown below:
1 mL = 10⁻³ L
Thus, volume = 42.0×10⁻³ L
Thus, moles of :
<u>Moles of = 0.0252 moles
</u>
According to the given reaction:
1 mole of reacts with 1 mole of
So,
0.019 mole of reacts with 0.019 mole of
Moles of = 0.019 mole
Available moles of = 0.0252 mole
<u>Limiting reagent is the one which is present in small amount. Thus, is limiting reagent.</u>
The formation of the product is governed by the limiting reagent. So,
1 mole of gives 1 mole of
0.019 mole of gives 0.019 mole of
Moles of formed = 0.019 moles
Molar mass of = 95.611 g/mol
Mass of = Moles × Molar mass = 0.019 × 95.611 g = 1.82 g
<u>1.82 g is the maximum mass of CuS.</u>
Answer: d. More than 6.5 grams of copper (II) is formed, and some copper chloride is left in the reaction mixture.
Explanation:
As can be seen from the chemical equation, 2 moles of aluminium react with 3 moles of copper chloride.
According to mole concept, 1 mole of every substance weighs equal to its molar mass.
Aluminium is the limiting reagent as it limits the formation of product and copper chloride is the excess reagent as (14-7.5)=6.5 g is left as such.
Thus 54 g of of aluminium react with 270 g of copper chloride.
1.50 g of aluminium react with=of copper chloride.
3 moles of copper chloride gives 3 moles of copper.
7.5 g of copper chloride gives 7.5 g of copper.