Answer:
The number of moles of H₂O is 0.135 mol.
The number of moles of LiClO₄ is 0.0449 mol.
Explanation:
Mole is an important standard unit used for the measurement of large quantities of atoms, molecules, or other particles. One mole is equal to 6.022×10²³ units.
The number of moles of a substance is calculated by:
To find the number of moles of H₂O:
Mass of H₂O in the sample = 2.43g
The molecular weight of H₂O = 18.02g
Number of moles = 
= 0.135 mol.
To find the number of moles of LiClO₄:
Mass of LiClO₄ given = 4.78g
The molecular weight of LiClO₄ = 106.39g
Number of moles = 
= 0.0449 mol.
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Answer:
An insulated beaker with negligible mass contains liquid water with a mass of 0.205kg and a temperature of 79.9 °C How much ice at a temperature of −17.5 °C must be dropped into the water so that the final temperature of the system will be 31.0 °C? Take the specific heat for liquid water to be 4190J/Kg.K, the specific heat for ice to be 2100J/Kg.K, and the heat of fusion for water to be 334000J/kg.
The answer to the above question is
Therefore 0.1133 kg ice at a temperature of -17.5 ∘C must be dropped into the water so that the final temperature of the system will be 31.0 °C
Explanation:
To solve this we proceed by finding the heat reaquired to raise the temperature of the water to 31.0 C from 79.9 C then we use tht to calculate for the mass of ice as follows
ΔH = m×c×ΔT
= 0.205×4190×(79.9 -31.0) = 42002.655 J
Therefore fore the ice, we have
Total heat = mi×L + mi×ci×ΔTi = mi×334000 + mi × 2100 × (0 -−17.5) = 42002.655 J
370750×mi = 42002.655 J
or mi = 0.1133 kg
Therefore 0.1133 kg ice at a temperature of -17.5 ∘C must be dropped into the water so that the final temperature of the system will be 31.0 °C
Solid substances cannot raise to the top of the ‘card’. They need to be in liquid form.
