What amount of heat (in kJ) is required to convert 10.1 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)

Two 20.0 g ice cubes at -17.00C are placed into 470.1 g of water at 25.0 0C. The heat of fusion of ice is 6.008 kJ/mol, the molar heat capacity of water is 75.3 J mol-1 K-1 and the molar heat capacity of ice is 37.7 J mol-1 K-1. Assuming no energy is transferred to or from the surroundings, please calculate the final temperature of the water after all the ice melts. _______ 0C

Liquid butane is used in cigarette lighters. The boiling point of butane at 1 atm pressure is -1.0 °C and its ∆H(vap) is 22.44 kJ/mol. R = 8.314 ×10⁻³ kJ/mol･K. Calculate the pressure (in atm) of the butane in the lighter at 19.5 °C.

Ethanol (C₂H₂OH) meits at-114 °C and boils at 78°C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 and 2.3 J/(g-K), respectively. Y Part A How much heat is required to convert 30.5 g of ethanol at 28 °C to the vapor phase at 78 "C? Express your answer in kilojoules to three significant figures. 195] ΑΣΦ Submit Part 8 Request Answer Submit ? How much heat is required to convert 30.5 g of ethanol at-160 C to the vapor phase at 78 "C7 Express your answer in kilojoules to two significant figures. VA24 Request Answer kJ kJ