A liquid is placed in an apparatus for measuring vapor pressure over a liquid. The results of 2 pressure-temperature measurements are P=239.9 mmHg at 357.1 K and P = 13.80 mmHg at 294.1 K. If these points fall on the straight-line plot of ln P vs 1/T, calculate the heat of vaporization of the substance. (Final answer in 4 decimals)

Based on the actual value for AHvap of water, how many kJ of energy are needed to convert 5.00 kg of water into steam at 100 °C? 2.

Using the information below, calculate how much energy (in kJ) is released when 12.0 g of water vapor at 113.0 ºC is cooled to 100 ºC and then condensed, GFM = 18.016 g/mol. Show all work and report you final answers to the correct units and significant figures. For H2O:  Cs = 2.03 J/(g·°C)     △Hfus = 6.02 kJ/mol                 Cl = 4.18 J/(g·°C)      △Hvap = 40.7 kJ/mol                  Cg = 2.0 J/(g·°C)

You perform a distillation of a certain liquid at two different pressures The first distillation was done on a day when the pressure was 760 mmHg .   The boiling point (the range where we saw drips come over) is 382.  This is in Kelvin. (This is the normal boiling point of that liquid) Then you connected the adapter to a vacuum.    The liquid now boils at 345 Kelvin.  The enthalpy of vaporization in kJ/mol is 18.5   What is the pressure of the vacuum in mm Hg ?   Hint: Clausius Clapeyron equation ln(P2/P1) =DHvap/R  * (T2-T1)/(T2T1)   or  ln(P2/P1) =DHvap/R  * (1/T1 - 1/T2)   R = 8.3145 J/mol K

Substance X is known to exist at 1atm in the solid, liquid, or vapor phase, depending on the temperature. Additionally, the values of these other properties of X have been determined (picture). You may also assume X behaves as an ideal gas in the vapor phase. Suppose a small sample of X at -20°C is put into an evacuated flask and heated at a constant rate until 10 kJ/mol of heat has been added to the sample. Graph the temperature of the sample that would be observed during this experiment.

Q1.)Using the data provided in Table 3 in the handout (also provided below), calculate the vapor pressure of water at 21.0 °C.?? Table 3:  Vapor pressure of water at various temperatures T (˚C) P (mmHg) T (˚C) P (mmHg) T (˚C) P (mmHg) 0 4.58 16 13.63 26 25.21 5 6.54 18 15.48 28 28.35 10 9.21 20 17.54 30 31.82 12 10.52 22 19.83 40 55.3 14 11.99 24 22.38 50 92.5 PART B)  In the experiment, you wrap a piece of copper wire around your magnesium strip to suspend the magnesium inside the eudiometer. Why is copper wire a good choice for this task? MULTIPLE CHOICE :  A.It conducts electricity very well B. It reacts strongly with the acid C. It does not react with the acid D. It is much heavier than Mg

Please don't provide handwritten solution ....

What amount of heat (in kJ) is required to convert 10.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g. °C; specific heat capacity of gas = 0.932 J/g⋅ °C; AHvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3 °C)

How much energy will be released by cooling 28.2 grams of steam from 118°C to 37°C?   cice = 2.02 J/g·K; cwater = 4.184 J/g·K; csteam = 1.97 J/g·K; ΔHfusion = 333 J/g; ΔHvap = 2450 J/g

Enter your answer in the provided box. From the data below, calculate the total heat (in J) needed to convert 0.821 mol of gaseous ethanol at 300.0°C and 1 atm to liquid ethanol at 25.0°C and 1 atm: b.p. at 1 atm: 78.5°C Cgas: 1.43 J/g °C AHⓇ : 40.5 kJ/mol vap Cliquid 2.45 J/g.°C