How many joules of energy are required to melt 80g of silver.
To find the amount of energy required to melt a substance, we need to use the formula:
Q = m * ΔH
Where:
Q = amount of energy (in joules)
m = mass of the substance (in grams)
ΔH = molar enthalpy of fusion (in joules/gram)
First, we need to find the molar enthalpy of fusion (ΔH) for silver. The molar enthalpy of fusion is the amount of energy required to change one mole of a substance from a solid to a liquid state. For silver, the molar enthalpy of fusion is 11.3 kJ/mol, or 11.3 × 10^3 J/mol.
Next, we convert the mass of silver from grams to moles. To do this, we need the molar mass of silver. The molar mass of silver (Ag) is 107.87 g/mol.
80g of silver is equal to:
80g / (107.87 g/mol) = 0.74 moles of silver
Now, we can use the formula to calculate the amount of energy (Q) required to melt the silver:
Q = m * ΔH
Q = 0.74 moles * (11.3 × 10^3 J/mol)
Q = 8.36 × 10^3 J
Therefore, approximately 8.36 × 10^3 joules of energy are required to melt 80 grams of silver.