how much heat is required to melt 25.6g of solid diethyl ether(at its melting point)
196.1
2.95kg X 1000g/1kg x 1 mol/74.14g x 7.27kJ/1mol =289.2702 kJ = 2.89 x 10^2 kJ
^^disregard my answer! I posted to the wrong question ... I'm so sorry
bama
To determine the amount of heat required to melt a substance, you need to know its molar heat of fusion (ΔHfus) and the molar mass (M). Here's how you can calculate it step by step:
1. Find the molar mass (M) of diethyl ether (C4H10O):
- Carbon (C): 4 x 12.01 g/mol = 48.04 g/mol
- Hydrogen (H): 10 x 1.01 g/mol = 10.10 g/mol
- Oxygen (O): 1 x 16.00 g/mol = 16.00 g/mol
Total molar mass (M) = 48.04 g/mol + 10.10 g/mol + 16.00 g/mol = 74.14 g/mol
2. Determine the molar heat of fusion (ΔHfus) of diethyl ether:
The molar heat of fusion is the heat required to change one mole of a substance from a solid to a liquid at its melting point. For diethyl ether, the value is approximately 8.2 kJ/mol.
3. Convert the number of grams of diethyl ether (25.6 g) to moles:
Moles (n) = Mass (m) / Molar mass (M)
n = 25.6 g / 74.14 g/mol ≈ 0.3456 mol
4. Calculate the heat required using the formula:
Heat (Q) = Moles (n) x Molar heat of fusion (ΔHfus)
Q = 0.3456 mol x 8.2 kJ/mol ≈ 2.83 kJ
Therefore, approximately 2.83 kilojoules (kJ) of heat is required to melt 25.6 grams of diethyl ether at its melting point.