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 80. °C boiling point 125. °C enthalpy of fusion 7.00 kJ/mol enthalpy of vaporization 21.00 kJ/mol 2.20 g/cm³ (solid) density 1.60 g/mL (liquid) 34. J.K-1 'mol (solid) 1 heat capacity 24. J.Kmol 1 (liquid) 1 57. J.Kmol (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) 150- 140- 130- 120- 110- 100+ 90- 80- 70- 60- 50- 0 3 4 5 6 7 9 10 heat added (kJ/mol) G

How much heat energy is required to convert 39.6 g of solid ethanol at -114.5 °C to gaseous ethanol at 147.2 °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 2.45 J/g. °C, and that of gaseous ethanol is 1.43 J/g. °C. q= 4326.84 kJ

Calculate the amount of energy (in kJ) necessary to convert 497 g of liquid water from 0°C to water vapor at 182°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g °C, and for steam is 1.99 J/g °C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) kJ

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 30. °C boiling point 90. °C enthalpy of vaporization enthalpy of fusion 8.00 kJ/mol 29.00 kJ/mol 1.70 g/cm (solid) 1.50 g/mL (liquid) density 35. J·K 1- •mol (solid) heat capacity 45. J'K (liquid) "mol 55. 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 0 °C is put into an evacuated flask and heated at a constant rate until 15.0 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment.

carbon disulfide Cs2 has a heat of vaporization of 29,200 J/mol. at 268 K it has a vapor pressure of 1.0 X 10^2 mmHg. what is its vapor pressure at 301 K

1. Calculate the amount of heat (in kJ) released when converting 150.2 g of water to ice at -23 degrees Celsius.    2. A closed vessel of volume 10.0 L initially contains 1.303 g of water and no water vapor. Please calculate the mass of liquid water remaining once the system reaches equilibrium at 30 degrees Celsius. The vapor pressure of water at that temperature is equal to 0.0418 atm.   3. A person drinks four glasses of cold water (5 degrees C) every day. The volume of each glass is 195. mL. How much heat (in kJ) does the body have to supply to raise the temperature of the water to 37 degrees C (body temperature)?   4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O­2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction:                 N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l)   5. Consider the following chemical equation. CH4(g) + 2O2(g) à CO2(g) + 2H2O(l)                 Using the values in the table, calculate…

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How much energy would need to be added to 930.g of ice at 0.0°C to turn it into liquid water at 0.0°C ? 930. J O 3.89x103 J O 1.86x103 J O 2.10x106 J 3.12x105 J

Consider the phase diagram shown. What is the normal sublimation point at 1 atm? Pressure (not to scale) 72.9 atm 5.1 atm 1 atm O 0°C O 100°C -56.7 °C 31°C -78.5 °C SOLID LIQUID GAS -78.5 °C -56.7 °C Temperature (not to scale) 31 °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