A 90 g sample of a substance released 1.99 kJ of heat as it cooled from...
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?
How much heat (in kJ) is released when 125.0 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol ∙ °C), and the molar heat capacity of ice is 36.4 J/(mol ∙ °C).
Consider the following data for an unknown substance X: AHvap = 21.00 kJ/mol Specific heat capacity of liquid = 2.40 J/g. °C Boiling point = 70.0°C Molar mass=92.00 g/mol When the temperature of 1.000 mole of X(g) is lowered from 94.0°C to form X(1) at 46.0°C, 29.97 kJ of heat is released. Calculate the specific heat capacity of X(9). Specific heat capacity = J/g. °C Submit Answer Try Another Version 5 item attempts remaining
How much heat is released when 105 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol • °C), and the molar heat capacity of ice is 36.4 J/(mol • °C). A)347 kJ B)54.8 kJ C)319 kJ D)273 kJ
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...
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
A new substance evolves (-2.26) kJ of heat when 20.36 g it cools from 134.8oC to 30.1oC. What is the specific heat (in J/(g K)) of this substance?
A chemist carefully measures the amount of heat needed to raise the temperature of a 229.0 g sample of a pure substance from -2.8 °C to 15.1 °C. The experiment shows that 570. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. J.g?:K-1 x | ?
155 gas a5 points) A 5.00 g sample of water Vapor, initially at 155°C is cooled at atmospheric pressure, producing ice at -55.0 °C. Use the following data:(specific heat capacity of ice is 2.09 J/god specific heat capacity of liquid water is 4.18 J/g C; d specific heat capacity of water vapor is 1.84 J/g°C) heat of fusion of ice is 336 J/g heat of vaporation of water is 2260 J/g. Кир a) Draw the cooling curve for the problem....