How much heat must be added to 23.9 g of solid white phosphorus, P4 , at 24.1°C to give the liquid at its melting point, 44.1°C? The heat capacity of solid white phosphorus is 95.4 J/(K·mol); its heat of fusion is 2.63 kJ/mol. Heat = J

Based on the thermodynamic properties provided for water, determine the amount of energy released for 130.0  g of water to go from 89.0 °C to -12.0 °C.  Property Value Units Melting point 0.0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05  kg of water decreased from 117  °C to 56.5  °C.  Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C

With around 70% of ammonia produced industrially being used to make fertilizers. The specific heat capacity of liquid ammonia is 80.8 J/g*K while that of gaseous ammonia is 37.0 J/g*K. Given that the boiling point and enthalpy of vaporization of ammonia is -33.3°C and 23.5 kJ/mol, respectively, how much energy is required to heat 75 g of ammonia (17.03 g/mol) from the temperature of liquid nitrogen (-195.8°C) to room temperature (25.0°C)?

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

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 (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.

The vapor pressure of liquid carbon disulfide, CS2, is 100. mm Hg at 268 K. A 0.261 g sample of liquid CS2 is placed in a closed, evacuated 400. mL container at a temperature of 268 K. Assuming that the temperature remains constant, will all of the liquid evaporate? What will the pressure in the container be when equilibrium is reached? mm Hg

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.45  kg of water decreased from 109  °C to 40.5  °C.   Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C      kJ