2.54 × 10⁵ kJ of heat are required to fully melt a 0.834 m³ block of ice, with a density of 917 kg / m³.
What is melting?
Melting is a physical change in which solids turn into liquids.
- Step 1. Calculate the mass of ice.
We have a block of 0.834 m³ of ice with a density of 917 kg/m³.
0.834 m³ × 917 kg/m³ = 765 kg = 7.65 × 10⁵ g
- Step 2. Convert 7.65 × 10⁵ g to moles.
We will use the molar mass of water.
7.65 × 10⁵ g × (1 mol/18,02 g) = 4.24 × 10⁴ mol
- Step 3. Calculate the heat required to melt 4.24 × 10⁴ moles of water.
According to the thermochemical equation, 6.01 kJ are required to melt 1 mol of water.
4.24 × 10⁴ mol × (6.01 kJ/mol) = 2.54 × 10⁵ kJ
2.54 × 10⁵ kJ of heat are required to fully melt a 0.834 m³ block of ice, with a density of 917 kg / m³.
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