Ethanol (C2 H;OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid ethanol at -50 °C? O 3949 207.3 6.67 8.97 O -12.5

The following information is given for mercury, Hg, at 1 atm: boiling point = 357 °C specific heat liquid = 0.139 J/g°C In progress At a pressure of 1 atm, of 357 °C. AHvap (357 °C) = 59.3 kJ/mol kJ of heat are needed to vaporize a 49.0 g sample of liquid mercury at its normal boiling point

Two 20.0 g ice cubes at -17.0 °C are placed into 235 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H,O(s) 37.7 J/ (mol·K) heat capacity of H,O(1) 75.3 J/ (mol·K) T = enthalpy of fusion of H,O 6.01 kJ/mol

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