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There is a difference in the change in chemical potential over temperature (∂μ/∂T) when water changes state.
Find the difference in the process of
a) freezing and
b) boiling at normal pressure.
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- A certain liquid has a vapor pressure of 92.0 Torr92.0 Torr at 23.0 ∘C23.0 ∘C and 339.0 Torr339.0 Torr at 45.0 ∘C.45.0 ∘C. Calculate the value of Δ?∘vapΔ�vap∘ for this liquid. Calculate the normal boiling point of this liquid. (Please type answer)2. All liquids have characteristic vapor pressure that vary with temperature. The characteristic vapor pressure for pure water at 22°C is 19.827 mm Hg and at 30.0°C is 31.824 mm Hg. Use these data to calculate the change in enthalphy per mole for the vaporizationTo vaporize 45.0 g CCl4 requires 9.69 kJ at its normal boiling point of 76.7 oC and 1 bar pressure. Calculate the molar enthalpy of vaporization of CCl4 under these conditions.
- Calculate the difference in slope of the chemical potential against temperature on either side of (a) the normal freezing point of water and (b) the normal boiling point of water. The molar entropy change accompanying fusion is 22.0 J K−1 mol−1 and that accompanying evaporation is 109.9 J K−1 mol−1. (c) By how much does the chemical potential of water supercooled to −5.0 °C exceed that of ice at that temperature?What is the boiling point of water in a pressure cooker with a pressure of 2.00 atm? (The enthalpy of vaporization of water is 40.7 kJ mol–1 .)5) How many phases are present in the following systems? Also define each of the terminologies associated with the phase diagram. Cu(s) + H2O(g) CuO(s) + H2 (g) NH,C1 NH3 + HCI (3); ZnSO4 . 3H2O(s) + 2H2O(g) (s) (g) ZnSO4. 5H2O(s)
- (3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).The molar enthalpy of vaporization of water is Avap H = 40.65 kJ molat its normal boiling point. Use the Clausius-Clapeyron equation (given below) to calculate the vapor pressure of water at 105.96 °C. Assume Avan H does not depend on temperature. Give your answer in torr with at least one decimal place. dIn P dT RTWhat is the resulting temperature when 100 g of water at 75°C is mixed with 30 g of ice at 0 °C? Assume that all of the ice has melted. The specific heat of water is 4.184 J g-1 C°.-1 and the heat of fusion of ice is 335 J g-1.
- what quantity of heat would be evolved if 5.68g of liquid aluminum freezes at its normal freezing point?Determine the enthalpy of vaporization at 343.15 K for water. (Note: The heat of vaporization for water is known to be 40.79 kJ mol-1 at 273.15 K, the Cp of water (Liq) was determined to be 85.6 J K-1 mol-1 and the Cp of water (solid) was to be 54.35 J K-1 mol-1). Use the reaction below and give your final answer in kJ mol-1. H2O(solid, 273.15 K, 0.1 atm)--------H2O(liq, 273.15 K, 0.1 atm)How much heat (in kJ mol–1 to two decimal places) is required to melt 300.0 g of water (H2O; 18.02 g mol–1) at its melting point using the given enthalpy of fusion? ΔH=6.01 kJ mol−1