Using the data in the figure below, calculate the minimum mass (in grams) of propane, C₃H₈(g), that must be combusted to provide the energy necessary to convert 25.30 kg of ice at -15.00°C to liquid water at 80.00°C. The enthalpy of fusion of ice is 6.020 kJ/mol, and the heat capacities for H₂O(l) and H₂O(s) are 4.184 J/g･°C and 2.030 J/g･°C, respectively. (Assume the combustion of propane yields the H₂O product as a gas.)

The heat of fusion for a material can be found by AHfus = m x Cp x AT where AHfus is the heat of fusion per gram, m is the mass of the solid substance being melted, C, is the specific heat of the surrounding medium, and ATis the change in the temperature of the surrounding medium as the solid melts. Calculate the heat of fusion of a 10.00-g piece of Substance X. Use 4.18 J/g-° C as the specific heat, and assume a AT of 10.00 °C. Express your answer to three significant figures (units of J/g) 41.8 418 O 4.18

Calculate the heat absorbed when 35.39 g of some substance at 13.16°C is completely melted. The molar heat of fusion for the substacnce is 5.91kJ · mol, and the molar mass is 16.45g · mol Exproco

Suppose you have a perfectly insulated container holding 2.00 kg of liquid water at a temperature of 20.0°C. You also have a large supply of ice cubes which are stored at a temperature of-20.0°C. (a) What is the maximum mass of ice you can add to the water so that all of the ice melts? Assume no heat is lost to the environment. (b) Suppose you add twice the mass of ice that you found in part a. How much solid ice will remain once thermal equilibrium is reached?