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Using the result from question 11.2.3 and another point from the graph, estimate
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- How much energy is required to vaporize 41.4 g of dichloromethane (CH2Cl2) at its boiling point, if its ΔHvap is 31.6 kJ/mol? Group of answer choices 55.1 kJ 31.2 kJ 6.49 kJ 18.1 kJ 15.4 kJarrow_forwardWhat quantity of heat (in kJ) is evolved when 25.0 g H2O(g) at 125.0 °C is converted to H2O(l) at 35.0 °C? Helpful information:specific heat of steam = 2.03 J/g·°Cspecific heat of water = 4.184 J/g·°CHeat of vaporization of water = 2.26 x 103 J/gHeat of fusion of water = 334 J/garrow_forwardWhat is the enthalpy change for heating ice from -5°C to steam at 105°C? The answer here is 54.57 kJ/mol. How did that happen?Assume 1 mole of H2O=18.015g=mass of ice=mass of water=mass of steam a. 46.66 kJ/mol b. 54.19 kJ/mol c. 54.57 kJ/mol d. 47.04 kJ/molarrow_forward
- 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/molCliq = 2.16 J/g°CCgas = 1.29 J/g°CCsol = 1.65 J/g°CTmelting = -95.0°Carrow_forwardSodium chloride, the table salt (NaCl) is added in cooking to enhance the flavor of the food. When 8.6 g of NaCl are added in 167 mL of water at 25.0oC in a coffee-cup calorimeter, 669 J of heat are absorbed. (Assume that there is no change in volume, d=1.00 g/mL, specific heat=4.18 J/g.oC). Evaluate the equilibrium temperature (in oC).arrow_forward3.A 33.3 g hot piece of metal at 450K is placed in pure water that has a volume of 155.0 mL which has an initial temperature of 5.3° After five minutes, equilibrium is established. What is the final temperature of the water in Celsius if the metal has a specific heat 0.33 J/g°Carrow_forward
- Energy Constants for H2O334 J/g = Heat of Fusion (Hf)2260 J/g = Heat of Vaporization (Hv)2.11 J/goC = Specific Heat Capacity of solid water4.18 J/goC = Specific Heat Capacity of liquid water2.00 =J/goC = Specific Heat Capacity of water vaporFor each problem, sketch a temperature vs. time graph and solve. 3. A 12-oz can of soft drink (m = 340 g) at 28oC is placed in a freezer where the temperature is -12oC. How much energy must be removed from the soft drink for it to become ice at -12oC?arrow_forwardThe heat of fusion of acetic acid is 11.72 KJ/mol at the melting point 16.61°C. Calculate Kf for acetic acid.arrow_forwardAre the values of ΔHvap and ΔSvap for boiling water going to be positive or negative? Explain if these signs will be consistent for other boiling liquids.arrow_forward
- In an experiment, 10.0 g of ice at −20.0°C is converted into steam with a temperature of 110.0°C. How much energy is required for this process?[ΔHvap =2260J/g; ΔHfus =334 J/g; cp (ice) =2.06 J/(g ⋅°C); cp (water) =4.18 J/(g ⋅°C);cp (steam) =1.99 J/(g ⋅°C)]arrow_forward3.15 mol of an unknown solid is placed into enough water to make 150.0 mL of solution. The solution's temperature increases by 20.11°C. Calculate ∆H, in kJ/mol, for the dissolution of the unknown solid. (The specific heat of the solution is 4.184 J/g・°C and the density of the solution is 1.20 g/mL).?arrow_forwardCalculating ΔG under Nonstandard Conditions What is the free energy change for theprocess shown here under the specified conditions? 2NH3(g) ⟶ 3H2(g) + N2(g) ΔG°=33.0 kJ/mol T = 25 °C, PN2 = 0.870 atm, PH2 = 0.250 atm, and PNH3 = 12.9 atmarrow_forward
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