What is the mass percent of a solution of 7.6 grams sucrose in 83.4 grams of water
1 answer:
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Answer:
The correct options include choice 2, 3, and 6.
Explanation:
Density is identified as the mass of a substance per unit volume occupied by that substance.
The density remains constant for a given substance, regardless of variations in mass and volume hence it is considered an intensive property.
2. 20.2 g of silver in 21.6 mL of water and 12.0 g of silver also in 21.6 mL of water.
3. 15.2 g of copper in 21.6 mL of water and 50.0 g of copper in 23.4 mL of water.
6. 11.2 g of gold in 21.6 mL of water and 14.9 g of gold in 23.4 mL of water.
The same metals in both instances will yield consistent densities due to the fixed density of the metal.
Answer:
There are 5.5668 moles of water for every mole of CuSO₄.
Explanation:
The mass of anhydrous CuSO₄ is:
23.403g - 22.652g = 0.751g.
mass of crucible + lid + CuSO₄ - mass of crucible + lid
Given that the molar mass of CuSO₄ is 159.609g/mol, we calculate the moles:
0.751g × = 4.7052x10⁻³ moles CuSO₄
The mass of water in the initial sample is:
23.875g - 0.751g - 22.652g = 0.472g.
mass of crucible + lid + CuSO₄ hydrate - CuSO₄ - mass of crucible + lid
As the molar mass of H₂O is 18.02g/mol, we find the moles:
0.472g × = 2.6193x10⁻² moles H₂O
The mole ratio of H₂O to CuSO₄ is:
2.6193x10⁻² moles H₂O / 4.7052x10⁻³ moles CuSO₄ = 5.5668
This indicates there are 5.5668 moles of water per mole of CuSO₄.
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Answer:
Explanation:
Assuming all calculations occur at standard pressure and a temperature of -1.72°C :
Where
is the number of moles of hydrogen
is the mass of hydrogen
is the density of hydrogen