If 25.0 kJ of heat is lost by 0.500 mol of substance A initially at 110 °C, what is the final temperature of substance A? For substance A:  molar heat of vaporization = 43.4 kJ/mol  molar heat of fusion = 4.9 kJ/mol  molar heat capacity of the liquid = 112.4 J/mol·K  molar heat capacity of the gas = 37.12 J/mol·K Select one:   a. 78 °C b. 52 °C c. 83 °C

Please explain step by step (it would be helpful if you also graph it)

Substance X is known to exist at 1 atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined: melting point enthalpy of fusion - 10. °C boiling point 4.00 kJ/mol enthalpy of vaporization 30. °C 39.00 kJ/mol 3 1.60 g/cm³ (solid) 1 1 density 44. J.K ·mol (solid) 1.30 g/mL (liquid) 1 -1 heat capacity 64. J.K ·mol (liquid) 1 1 54. J.K mol (vapor) You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at -50 °C is put into an evacuated flask and heated at a constant rate until 10.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment. temperature (°C) 50- 40 30. 20 10. -10 -20 -30 -40 -50 0 1 2 3 4 5 6 7 8 9 10 heat added (kJ/mol) ☑ ? 00. 18 Ar

Compounds such as CCl2 F2 are known as chlorofluorocarbons, or CFCs. These compounds were once widely used as refrigerants but are now being replaced by compounds that are believed to be less harmful to the environment. The heat of vaporization of CCl2 F2 is 289 J/g.

How much heat energy is required to convert 44.9 g of solid ethanol at -114.5 °C to gasesous ethanol at 160.8 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of –114.5°C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45J/g · °C, and that of gaseous ethanol is 1.43J/g · °C. kJ

How much heat must be added to 100 g of ice at -5°C to turn it into 60 grams of water and 40 grams of steam, both at 100°C? Cp H2O = 75.7 J/mol-K, Cp Ice = 37.7 J/mol-K, Cp Steam = 35.1 J/mol-K, ΔHfus = 6.01 kJ/mol, ΔHvap = 40.7 kJ/mol

Consider the following data for an unknown substance X: AHvap 19.00 kJ/mol Specific heat capacity of liquid = 2.10 J/g °C Boiling point = 66.0°C Molar mass = 119.0 g/mol When the temperature of 1.000 mole of X(g) is lowered from 91.0°C to form X(1) at 41.0°C, 30.38 kJ of heat is released. Calculate the specific heat сараcity of X(g). Specific heat capacity = J/g °C Submit Answer Try Another Version 10 item attempts remaining 11 33°F 12 Tch

How much heat (in kJ) is released in converting 1.00 mol of water as a gas at 105°C to ice at –5.0°C? The heat capacity of H2O (g) is 2.01 J/g · °C The heat capacity of H2O (l) is 4.18 J/g · °C The heat capacity of H2O (s) is 2.09 J/g · °C The heat of fusion for water at 0 °C is approximately 0.334 kJ/g The heat of vaporization for water at 100 °C is 2.230 kJ/g.