Calculate the heat energy released when 19.0 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for mercury at 1 atm heat capacity of Hg(1) 28.0 J/(mol·K) kJ melting point 234.32 K * TOOLS enthalpy of fusion 2.29 kJ/mol x10

What amount of heat (in kJ) is required to convert 19.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g-°C; specific heat capacity of liquid = 1.58 J/g-°C; AHfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)

Calculate the heat energy released when 22.1 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for mercury at 1 atm 28.0 heat capacity of Hg(1) melting point enthalpy of fusion J/(mol-K) 234.32 K 2.29 kJ/mol 4p= kJ

Octane(C3H18) is a hydrocarbon found in crude oil. Thermochemical data for octane is provided below. The total change in enthalpy is 15.94 kJ when heating 0.2500 moles of octane from -70.00°C to 100.0°C. Determine the AHfusion. Melting point: -57.00 °C Boiling point: 126.0 °C J Csolid : 185.0 °C mol J Cliquid: 254.0 °C mol J Cgas: 250.0 °C mol AHvap: 34.40 kJ/ mol Molar mass: 114.23 g/mol 0.2693 kJ/mol 4.720 kJ/mol O 21.50 kJ/mol 0.2540 J/mol