How much energy in kilojoules is needed to heat 5.00 g of ice from -11.0 °C to °30.0 °C? The heat of fusion of water is 6.01 kJ>mol, and the m# olar heat capacity is 36.01 kJ>mol for ice and 75.4 J/K mol2 for liquid water

Specific heat capacity is the amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. For ice, this value is crucial for calculating the energy needed to increase its temperature from -11.0 °C to 0 °C before it melts. Understanding this concept allows us to quantify the energy changes associated with temperature changes in a substance.

The heat of fusion is the amount of energy required to change a substance from solid to liquid at its melting point without changing its temperature. For water, this value is 6.01 kJ/mol. This concept is essential for calculating the energy needed to melt the ice after it has reached 0 °C, as it represents the energy transition from solid ice to liquid water.

Phase changes refer to the transitions between solid, liquid, and gas states of matter, which occur at specific temperature ranges. In this problem, we need to consider the heating of ice, its melting into water, and then the heating of the resulting water. Understanding the different phases and the corresponding energy requirements for each phase change is vital for accurately calculating the total energy needed for the entire process.