How much heat energy is required to convert 65.6 g of solid iron at 27 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g. °C). q= kJ

The specific heat capacity of silver is 0.235 J/g. K. Its melting point is 962 °C, and its enthalpy of fusion is 11.3 kJ/mol. What quantity of energy, in joules, is required to change 5.20 g of silver from a solid at 25 °C to a liquid at 962 °C? Energy required: J =

Suppose 1.0 x 102 grams of ice absorbs 1255 J of heat, reaching a final temperature of -2.0°C.What was the initial temperature change of the ice? The specific heat capacity of H 2 O(s) = 2.1J/(g·ºC)

Calculate the energy released as heat when 18.7 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. heat capacity of Hg(1) Constants for mercury at 1 atm melting point enthalpy of fusion 28.0 J/(mol-K) # 234.32 K 2.29 kJ/mol 9 = MacBook Pro

The following information is given for cobalt at 1atm: boiling point = 3097°C AHvap = 6.60 kJ/g melting point = 1495°C AHfus = 263 J/g What is the energy change, Q, in kJ for the process of freezing a 39.8 g sample of liquid cobalt at its normal melting point of 1495°C. kJ

Consider the following data for ethanol, C2H5OH: Melting Point = -114°C Boiling Point = 78°C ΔHfusion = 5.0 kJ/mol ΔHvaporization = 42.6 kJ/mol Specific Heat of Liquid Ethanol = 2.5 J/g•°C Sketch a cooling curve that depicts ethanol vapor at 78°C being cooled until solid ethanol is formed at -114°C and then calculate the total amount of heat in kilojoules released when 55 grams of ethanol undergoes this process.

How much heat energy is required to convert 77.6 g of solid iron at 21 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g · °C). q= kJ

From 25.0°C to 94.5°C, 75.1 grams of ethanol are heated. What was the energy requirement in joules?H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. cp (liquid) ethanol 2.46 J/g°C, cp (gas) ethanol 1.43 J/g°C, and cp (solid) ethanol 2.42 J/g°C are the specific temperatures for the three phases of ethanol. Ethanol has a molecular weight of 46. The melting point of ethanol is -114.1 °C and the boiling point is 78.4 °C.

Calculate the amount of heat (in kJ) required to raise the temperature of a 86.0 g sample of ethanol from 198.0 K to 300.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. 60.0 kJ 21.2 kJ 11.9 kJ 75.6 kJ 28.4 kJ

A sample of C3H4Br2 has a normal boiling temperature of 131.5 °C. The enthalpy of vaporization for this compound is 35.4 kJ/mol. How much energy would be required to heat a 13.5 gram sample of liquid C3H4Br2 from 97.5 °C to a gas at 187.2 °C? The specific heat for the liquid is 0.865 J/g °C and the specific heat for the gas is 0.364 J/g. °C.