Consider the heating curve provided for 1.00 mole of a substance that begins as a solid at -14.8 °C and ends as a gas at 121.1 °C. Specific heat capacities: solid = 145.6 J/mol･ °C, liquid = 97.25 J/mol･ °C, gas = 68.49 J/mol･ °C
Step A: What quantity of heat energy (in kJ) must be absorbed to increase the temperature of the solid from -14.8 °C to the melting temperature?
Step B: What quantity of heat energy (in kJ) must be absorbed to melt the solid?
Step C: What quantity of heat energy (in kJ) must be absorbed to increase the temperature of the liquid from the melting temperature to the boiling temperature?
Step D: What quantity of heat energy (in kJ) must be absorbed to boil the liquid?
Step E: What quantity of heat energy (in kJ) must be absorbed to increase the temperature of the gas from the boiling temperature to the final temperature of 121.1 °C?
Step F: What is the total amount of energy that must be absorbed for the entire process?