determine the amount of heat, in kJ required to heat 69 g of solid Ca at 851C to 1,994 C
determine the amount of heat, in kJ required to heat 69 g of solid Ca at...
Determine the amount of heat, in kJ, required to heat 41 g of solid Ca at 851C to 1,397 C. Melting Point = 851C Boiling Point = 14870 Molar Heat Capacities: Csolid = 26.2 J/mol C Cliquid = 31.0 J/mol AH_fusion = 9.33 kJ/mol AH_vaporization = 162 kJ/mol Determine the amount of heat, in kJ, required to convert 24 g of solid Ca at 116 C to its melting point of 851C. Melting Point = 851C Boiling Point = 1487C...
Determine the amount of heat, in kJ, required to melt 33 g of solid Ca at its melting point of 851C. Melting Point = 851C Boiling Point = 1487C Molar Heat Capacities: Csolid = 26.2 J/mol C C liquid = 31.0 J/molC ΔH_fusion = 9.33 kJ/mol ΔH_vaporization = 162 kJ/mol
Determine the amount of heat, in kJ, required to heat 16 g of solid Ca at 851C to 1,375 C. Melting Point = 851C Boiling Point = 1487C Molar Heat Capacities: Csolid = 26.2 J/mol C C liquid = 31.0 J/molC ΔH_fusion = 9.33 kJ/mol ΔH_vaporization = 162 kJ/mol
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
Using the provided data, calculate the amount of heat, in kJ, required to warm 21.7 g of solid water, initially at -10. °C, to gaseous water at 112. °C. water molar mass 18.0153 g/mol melting point 0. °C boiling point 100. °C ΔHfus 6.02 kJ/mol ΔHvap at bp 40.7 kJ/mol Cs, solid 2.09 J/g⋅°C Cs, liquid 4.18 J/g⋅°C Cs, gas 1.87 J/g⋅°C 72.4 kJ 57.6 kJ 58.5 kJ 66.3 kJ 13.9 kJ
Using the provided data, calculate the amount of heat, in kJ, required to warm 22.3 g of solid acetone, initially at -110. °C, to gaseous acetone at 74. °C. acetone molar mass 58.0791 g/mol melting point -95. °C boiling point 56. °C ΔHfus 5.69 kJ/mol ΔHvap at bp 29.1 kJ/mol Cs, solid 1.6 J/g⋅°C Cs, liquid 2.16 J/g⋅°C Cs, gas 1.47 J/g⋅°C
Determine the amount of heat energy (in kJ) needed to warm a 58.5-g sample of ethanol (C2H5OH) from-150°C to 55°C. C2H5OH 46.07 g/mol AHvap 38.56 kJ/mol ΔΗrus 4.90 kJ/mol Boiling Point 78.5°C Freezing Point -117.3°C Specific Heat Capacity (c) of solid 0.249 J/g.°C Specific Heat Capacity (c) of liquid 2.44 J/g.°C Specific Heat Capacity (c) of gas 1.70 J/8.°C
PartA Calculate the amount of heat required to completely sublime 97.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol. Part B How much heat is evolved in converting 1.00 mol of steam at 155.0 ∘C to ice at -55.0 ∘C? The heat capacity of steam is 2.01 J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).
Calculate the amount of heat in kJ that is required to heat 20.0 g of ice from -25 ºC to 90 ºC, and sketch a heating curve for the process. The specific heat of ice is 2.11 J/( g. ºC); water 4.18 J/( g. ºC) and the ΔHfus for water is 6.01 kJ/mol