You have a 10.0 g sample of water at 373 K. How much energy must you...
How much energy is required to heat 36.0 g H2O from a liquid at 65°C to a gas at 115°C? The following physical data may be useful. ΔHvap = 40.7 kJ/mol Cliq = 4.18 J/g°/sup>C Cgas = 2.01 J/g°/sup>C Csol = 2.09 J/g°/sup>C Tmelting = 0°/sup>C Tboiling = 100°/sup>C
How much energy must be removed from a 94.4 g sample of benzene (molar mass= 78.11 g/mol) at 322.0 K to solidify the sample and lower the temperature to 205.0 K? The following physical data may be useful. ΔHvap = 33.9 kJ/mol ΔHfus = 9.8 kJ/mol Cliq = 1.73 J/g°C Cgas = 1.06 J/g°C Csol = 1.51 J/g°C Tmelting = 279.0 K Tboiling = 353.0 K
Question 3 7.5 pts How much energy must be removed from a 22.2 g sample of benzene CH) at 85.0°C to solidify the sample and lower the temperature to -7.5°C? The following physical data may be useful. AHvap = 33.9 kJ/mol AHfus = 9.8 kJ/mol Cliquid - 1.73J/gºC Cgas = 1.06 J/g°C Csolid - 1.51 J/g°C Tmelting = 6,0 °C Tboiling = 80.0°C 29.4 kJ 15.8 kJ O 17.6 kJ O 70.2 kJ 10.5 kJ
How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The following physical data may be useful. ΔHfus = 7.27 kJ/mol Cliq = 2.16 J/g°C Cgas = 1.29 J/g°C Csol = 1.65 J/g°C Tmelting = -95.0°C
How much energy (heat) is required to convert 52.0 g of ice at -10.0 C to steam at 100 C?Specific heat of ice: 2.09 J/g * C DHfus = 6.02 kJ/molSpecific heat of water: 4.18 J/g * C DHvap = 40.7 kJ/molSpecific heat of steam: 1.84 J/g * C
23. The enthalpy change for converting 10.0 g of water at 25.0eC to steam at 135.0eC is kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H20, AHius = 6.01 kJ/mol, and AHvap = 40.67 kJ/mol ku. 24. The enthalpy change for converting 1.00 mol of ice at -50.0eC to water at 70.0e is The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K,...
how much heat is released when 10.0 g of steam (water vapor ) at 105.0 C is cooled to liquid water at 25 C? S(water) = 4.18 J/g.C. ... S(steam) = 2.01 j/ g.C the heat of fusion of water is 6.02 KJ/ mol. The heat of vaporization of water is 40.7 KJ/mol
Only do question 4-6 show all work CHM 107, Quiz 1 Name How much energy must be removed from a 125 g sample of benzene (CH6 vapor at 425.0 K to make it a solid at 200.0 K? Use the following steps to get to your answer. You MUST show your work to receive any credit. The following physical data for benzene may be useful. See announcement for due date. AHvap 33.9 kJ/mol Cliq 1.73 J/g C Cgas 1.06 Csol...
Question 10 0.5 pts Consider the heating curve of water below. What is the energy change (in kJ) when 38.5 g of water vapor (or steam) at 135°C is cooled to 95°C? Hint: Cice = 2.09 J/(g•°C), Cwater = 4.18 J/(g°C), Csteam = 2.00 J//goºC) Hint: A Hus = 6.02 kJ/mol, AHvap = 40.7 kJ/mol 140°C - Temperature 100°C 0°C -100 +93.5 -90.6
How much heat (in kJ) is required to warm 10.0 g of ice, initially at -10.0 ∘C, to steam at 112.0 ∘C? The heat capacity of ice is 2.09 J/g⋅∘C and that of steam is 2.01 J/g⋅∘C.