A 357.7-gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C to 51.8 °C. (heat capacity of solid = 2.96 J/g・°C; heat capacity of liquid = 1.75 J/g・°C; ∆Hfus = 8.04 kJ/mol; Tf = 17.6 °C)
A.) How much Energy (in KJ) is absorbed/released to heat the solid?
B.) How much energy (in KJ) is absorbed/ released to melt solid?
C.) How much energy (in KJ) is absorbed/ released to heat the liquid?
D.) What is the total amount of energy that must be absorbed/released for the entire process
A 357.7-gram sample of an unknown substance (MM = 92.41 g/mol) is heated from -23.1 °C...
please help!!!! A 272.3 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity of liquid = 1.62 J/g. °C; heat capacity of gas = 1.04 J/g. °C; AHvap = 78.11 kJ/mol; Tb = 160.3 °C) How much energy (in kJ) is absorbed/released to cool the gas? pple A 272.3 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity...
A 233.9 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 °C to 147.6 °C. (heat capacity of liquid = 1.62 J/g. °C; heat capacity of gas = 1.04 J/g. °C; AHvap = 78.11 kJ/mol; Tb = 160.3 °C) How much energy (in kJ) is absorbed/released to condense the gas?
What amount of heat (in kJ) is required to convert 10.1 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (heat capacity of solid = 2.39 J/g・°C; heat capacity of liquid = 1.58 J/g・°C; ∆Hfus = 3.72 kJ/mol; Tf = 10.3°C)
What amount of heat (in kJ) is required to convert 26.1 g of an unknown solid (MM = 67.44 g/mol) at -15.4 °C to a liquid at 42.7 °C? (heat capacity of solid = 1.95 J/g・°C; heat capacity of liquid = 1.18 J/g・°C; ∆Hfus = 5.72 kJ/mol; Tf = 28.3°C) NOTE: The answer is NOT 4.99
How much heat is required to raise a 5.38 g sample of aluminum (26.98 g/mol) from 29.0°C to a temperature of 894°C? The information below may be useful. Specific heat capacity of Al (solid) = 0.903 J/g x *C Specific heat capacity of Al (liquid) = 1.18 J/g x *C ΔHfusion = 10.7 kJ/mol Melting Point of Al = 660*C
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...
How much energy (in kilojoules) is released when 12.6 g of steam at 110.5 ∘C is condensed to give liquid water at 67.0 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor.
How much heat energy is required to convert 45.2 g of a solid iron at 28 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). Question 6 of 6 > How much heat energy is required to convert 45.2 g of solid iron at 28 °C to liquid iron at...
The following information is given for lead at latm: AH yap(1740 °C) -178 kJ/mol AH fus(328 °C) = 4.77 kJ/mol boiling point = 1740 °C melting point = 328 °C specific heat solid= 0.130 J/gºC specific heat liquid = 0.138 J/gºC What is AH in kJ for the process of freezing a 26.3 g sample of liquid lead at its normal melting point of 328 °C. The following information is given for silver at latm: AHvap(2212 °C) = 254 kJ/mol...
A 61.93 gram sample of iron (with a specific heat of 0.450 J/g °C) is heated to 100.0 °C. It is then transferred to a coffee cup calorimeter containing 40.6 g of water (specific heat of 4.184 J/ g °C) initally at 20.63 °C. If the final temperature of the system is 23.59, what was the heat absorbed (q) of the calorimeter? (total heat absorbed by the water and calorimeter = heat released by the iron)