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The vapor pressure of ethanol is \(1.00 \times 10^{2} \mathrm{mmHg}\) at \(34.90^{\circ} \mathrm{C}\). What is its vapor pressure at \(63.16^{\circ} \mathrm{C}\) ? ( \(\mathrm{AH}_{\text {vap }}\) for ethanol is \(39.3 \mathrm{~kJ} /\) mol. )
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Calculate the amount of energy (in kJ) necessary to convert \(457 \mathrm{~g}\) of liquid water from \(0^{\circ} \mathrm{C}\) to water vapor at \(187^{\circ} \mathrm{C}\). The molar heat of vaporization \(\boldsymbol{H}_{\mathrm{vap}}\) ) of water is \(40.79 \mathrm{~kJ} / \mathrm{mol}\). The specific heat for water is \(4.184 \mathrm{~J} / \mathrm{g} *{ }^{\circ} \mathrm{C}\), and for steam is \(1.99 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\). (Assume that the specific heat values do not change over the range of temperatures in the problem.)
\(\mathbf{k} \mathbf{J}\)
Please post Q2 as a new question
The vapor pressure of ethanol is 1.00 × 102 mmHg at 34.90°C. What is its vapor pressure at 61.25°C? (ΔHvap for ethanol is 39.3 kJ/mol.) (answer in mmHg)
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The vapor pressure of ethanol is 1.00 x 102 mmHg at 34.90 degrees C. What is its vapor pressure at 62.17 degrees C? (Hvap for ethanol is 39.3 kJ/mol)
The vapor pressure of ethanol is 1.00 x 102 mmHg at 34.90oC. What is its vapor pressure at 51.73 oC? (ΔHvap for ethanol is 39.3 Kj/mol.) Given the vapor pressure at one temperature, P1, we can calculate the vapor pressure at a second temperature, P2. In (P1/P2) = ΔHvap/R (1/T2 - 1/T1) Where, ΔHvap for ethanol must have the units of J/mol. R = 8.314 J/K.mol .. The temperatures must be in Kelvins. Solve for P2, What is the vapor...
Can someone help me with this 10. -15 points ChangE7 12.PE.005. The vapor pressure of ethanol is 100 mmHg at 34.9°C. What is its vapor pressure at 47.5°C (Avap for ethanol is 39.3 kJ/mol.) mmHg
Calculate the amount of energy (in kJ) necessary to convert 557 g of liquid water from 0C to water vapor at 182C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g C, and for steam is 1.99 J/g C. (Assume that the specific heat values do not change over the range of temperatures in the problem.)
Calculate the amount of energy (in kJ) necessary to convert 557 g of liquid water from 0°C to water vapor at 172°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g ·°C, and for steam is 1.99 J/g ·°C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) = KJ
At what temperature does ethanol boil on a day in the mountains when the barometric pressure is 547 mmHg? The heat of vaporization of ethanol is 39.3 kJ/mol and its normal boiling point is 78.3°C. (R = 8.314 J/K • mol) 4) Draw the phase diagram for a substance that liquifies with increasing pressure.