Research the melting point, boiling point, heat of fusion, heat of vaporization, and heat capacity values...
How much heat energy is required to convert 15.0 g of solid ethanol at -114.5 °C to gasesous ethanol at 143.1 °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. How much heat energy...
The specific heat of CCl4(l) is 0.857 J/(g ∙ °C) its heat of fusion is 3.27 kJ/mol and its heat of vaporization is 29.82 kJ/mol. 1.Calculate the total quantity of heat required to convert 35.0 g of liquid CCl4 (MW: 153.81g/mol) from 25.0°C to become completely gaseous CCl4 at its boiling point of 76.8°C. 2. Sketch the heating curve for this compound, be sure to label the axes, the Tm, Tb, Hvap, and Hfus.
The heat of vaporization of benzene (C6H6) is 30.77 kJ/mol at it's boiling point (80 C). As a liquid, it has a heat capacity of 134.8 J/mol*K, and as a gas it has a heat capacity of 82.4 J/mol*K. Calculate the enthalpy change of heating 245g of benzene from 50 C to 100 C.
potassium metal has melting point of 63.65 C and a boiling point of 774 C Enthalpy fusion = 14.37 cal/g enthaply of vaporization = 490.3 cal/g Specific heat @ solid = .1759 cal/gC specfic heat @ liquid =.5425 cal /gC specfic heat @ gas = .2629 cal /gC a) draw heatung curve that us heated from 23C to 1200c b) Calculate total heat required in units of kJ for 39.5 g of potassium
Methylene chloride has a melting point of - 94.8°C, a boiling point of 40.0°C, a specific heat of 1.21 J/g *K for the solid and liquid, and 0.608 J/g*K for the gas. The heats of fusion and vaporization are ΔHfus of 73.40 J/g, and ΔHvap of 334.35 J/g respectively. Determine how many joules of energy are needed to heat 40 grams of methylene chloride from -171.4 ° F to 333 K. Draw out and label your heating curve. This will...
How much heat energy is required to convert 19.8 g of solid ethanol at –114.5 °C to gasesous ethanol at 175.0 °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.
How much heat energy is required to convert 49.7 g of solid ethanol at –114.5 °C to gasesous ethanol at 135.5 °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. kᎫ
How much heat energy is required to convert 16.2 g of solid ethanol at -114.5 °C to gasesous ethanol at 191.9 °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.
How much heat energy is required to convert 55.6 g of solid ethanol at -114.5 °C to gasesous ethanol at 165.9 °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.
Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 degrees Celsius. What is the vapor pressure of ethanol at 15 degrees Celsius?