The following is a table of water vapor pressure in millibar (mbar) vs Temp in °C. In your own words, explain what equilibrium this represents, making sure to include an equation, and why it changes with temperature. T (°C) P (mbar) 15 17.1 16 18.1 17 19.3 18 20.7 19 22.0 20 23.3 21 24.9 22 26.4 23 28.1 24 29.9 25 31.7 26 33.6 27 35.6 28 37.7 29 40.0 30 42.4

The question is in the image. Additional information: Explain why it shifts that way.

h hydrogen sulfide (H₂S) is usually extracted from 'sour' natural gas, it can also be produced directly from gaseous hydrogen and sulfur at high temperatures: File Preview 2H₂(g) + S₂(g) → 2H₂S(g) In one experiment, 1.20 atm of H₂ and 0.720 atm of S₂ were put in an evacuated cylinder. At equilibrium, the total pressure of the system was 1.47 atm. What is equilibrium constant, Kp, for the reaction?

A 650 mL reaction vessel initially contains 0.0125 mol of H,S at 800 °C. Calculate partial pressure of H, at equilibrium. 2 H2S (g) = 2 H2 (g) + S2(g) Kc = 1.67x107 at 800 °C 1 atm = 760 mmHg = 760 torr = 1.013 bar R = 0.08206 L atm mol-1 K-1 = 8.314 J mol-1 K-1 31.4 mmHg 16.7 mmHg 33.3 mmHg 46.2 mmHg 62.9 mmHg

olo While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 200. mL flask with 3.8 atm of ethylene gas and 1.5 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 2.96 atm of ethylene gas and 0.66 atm of water vapor. The engineer then adds another 0.95 atm of ethylene, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm

While ethanol (CH3CH2OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH2CH2) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 5.0 L flask with 1.0 atm of ethylene gas and 3.0 atm of water vapor. When the mixture has come to equilibrium he determines that it contains 0.58 atm of ethylene gas and 2.58 atm of water vapor. The engineer then adds another 1.0 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. atm x10 E

68. The vapor pressure of butyl alcohol (C4H,OH) at 70.1°C is 0.1316 atm; at 100.8°C, it is 0.5263 atm. (a) Calculate the molar enthalpy of vaporization (AHvap) of butyl alcohol. (b) Calculate the normal boiling point of butyl alcohol.

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas wi form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 500. ml. fask with 3.2 am of carbon monoxide gas and 25 atm of water vapor. When the mixture has come to equilibrium he determines thatit contains 1.5 aem of carbon monoxide gas, 0.80 atm of water vapor and 1.7 atm of hydrogen gas The engineer.then adds another 13 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of carton dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm

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