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It is a hot summer day, and Chris wants a glass of lemonade. There is none in the refrigerator, so a new batch is prepared from freshly squeezed lemons. When finished, there are
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- Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forward9.91 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g・ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. my answer -38.99 kJ/mol was wrong.arrow_forward10.71 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g・°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.arrow_forward
- A constant pressure calorimeter contains 286 g of water at 20.0 °C. A 13.41 g of substance X (molar mass 154 g/mol) at 20.0°C was dissolved in this water. The temperature of the solution increased to 23.5 °C. Assuming the specific heat of the mixture is 4.184 J g‑1°C‑1, and the density of the solution is 1.00 g/cm3, calculate the enthalpy change (in kJ) for the dissolution of 1 mole of X.arrow_forward7.16 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g・°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water. A 44.0 g sample of an unknown metal at 100.0 °C is placed in a constant pressure calorimeter containing 80.0 g of water at 24.8 °C. The final temperature is 28.4 °C. Assume that the heat capacity of the calorimeter equals the heat capacity of the water it contains. Calculate the specific heat capacity of the metal and use the result to identify the metal.arrow_forwardA coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 185.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 °C to 23.74 °C. Calculate the enthalpy of solution, AHgoln , per mole of salt dissolved. Assume the specific heat of the solution is 4.12 J/(g.°C) and the heat capacity of the calorimeter is 4.10 J/ °C. Calculate the heat change experienced by the calorimeter contents, Icontents · Icontents J Calculate the heat change experienced by the calorimeter, qcal - Ical = J Calculate the heat change produced by the solution process, Isoln · Activate Windowsarrow_forward
- 3. A 262-mL sample of a sugar solution containing 1.22 g of the sugar has an osmotic pressure of 30.3 mmHg at 35°C. Determine the molar mass of the sugar. (1 mmHg = 0.00131atm) A 4.117-g impure sample of glucose (C&H12O6) was burned in a constant-volume calorimeter having a heat capacity of 19.65 kJ/°C. If the rise in temperature is 3.134°C, calculate the percent by mass of the glucose in the sample. Assume that the impurities are unaffected by the combustion process. b)arrow_forwardA coffee cup calorimeter was used to measure the heat of solution, the change in enthalpy that occurs when a solid dissolves in water. A 10.0 g sample of an ionic compound with a molar mass of 145.0 g/mol was added to a sample of deionized water to produce 60.0 grams of solution. After stirring and dissolving the solid, the temperature was found to change from 25.00 °C to 23.71 °C. Calculate the enthalpy of solution, AH30ln , per mole of salt dissolved. Assume the specific heat of the solution is 4.15 J/(g.C) and the heat capacity of the calorimeter is 5.30 J/°C. Calculate the heat change experienced by the calorimeter contents, qcontents - 9contents = J Calculate the heat change experienced by the calorimeter, qcal - 9cal = J Calculate the heat change produced by the solution process, qsoln - Isoln = J Calculate AHsoln , the enthalpy of solution for one mole of solid in kilojoules per mole. ΔΗon= kJ/molarrow_forward
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