Given the AG1000 gas-phase values 84.31 kcal/mol for n-pentane, 83.64 kcal/mol for isopentane, and 89.21 kcal/mo for neopentane, find the mole fractions present in an equilib- rium mixture of these gases at 1000 K and 0.50 bar.
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- Acetyl Salicylate, C9H8O4, reacts with Potassium hydroxide. 1.75g of acetyl salicylate were hydrolyzed with 50cm3 of 0.57mol/dm3 of potassium hydroxide and the mixture were made up of 250cm3 with distilled water in a volumetric flask. Calculate: The number of moles of acetyl salicylate in 1.75g The number of moles of potassium hydroxide of 0.575mol/dm3 solution. The molarity of excess potassium hydroxide in the 250cm3 solution. If 1.15g of salicylic acid, C7H8O3, were obtained. Determine the percentage yield of the reaction.Calculate the values for log Kow and the saturated aqueous solubility (Cw$sat) for bisphenol A. The value for log Kow is 3.62 ; enter your answer as X.XX The value for Cwsat is ; report your answer in units of moles/liter and enter it as X.XX×10(-X). Bisphenol A is closest to "phthalates" H3C CH3 HO HO,Calculate the value of the equilibrium constant, Ke , for the reaction Q(g)+X(g) = 2 M(g)+N(g) given that M(g) Z(g) 6 R(g) = 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) 9R(g) Kei 3.59 Kc2 0.567 Kc3 = 13.8 K. =
- › Calculate the value of the equilibrium constant, Kỵ, for the reaction Q(g) + X(g) — 2M(g) + N(g) given that Kc = M(g) — Z(g) 6R(g) 2 N(g) + 4 Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kc1 = 3.48 Kc2 Kc3 = 0.587 = = 13.6Henry s law is important in environmental chemistry, where it predicts the distribution of pollutants between water and the atmosphere. The hydrocarbon methylacetylene (C3H4) emitted in wastewater streams, for example, can pass into the air, where it is degraded by processes induced by light from the sun. The Henry s law constant for methylacetylene in water at 25 °C is 601 atm, when the following form of the law is used: = k methylacetylene Calculate the partial pressure of methylacetylene vapor in equilibrium with a solution of 1.47 g of methylacetylene per 1060 L of water. How many methylacetylene molecules are present in each cubic centimeter of vapor? P methylacetylene methylacetylene methylacetylene X = atm molecules per cubic centimeterCalculate the value of the equilibrium constant, Ke , for the reaction Q(g) + X(g) = 2 M(g) + N(g) given that M(g) = Z(g) 6 R(g) = 2 N(g) + 4Z(g) 3 X(g) + 3 Q(g) = 9R(g) Kel = 3.52 K2 = 0.585 Kc3 12.3 K. II
- Calculate the masses of oxygen and nitrogen that are dissolved in 3.0 L of aqueous solution in equilibrium with air at 25 °C and 760 Torr. Assume that air is 21% oxygen and 78% nitrogen by volume. 0.55104 mass: Henry's law constants for gases in water at 25 °C Gas kn (bar-M-¹) He 2.7 x 10¹ N₂ 1.6 x 10' 0₂ 7.9 x 10² CO₂ 29 H₂S 10. 1.79 source: S, Rock, And Gallogly 46-General Chemistry | Publisher: University BooksNeed help with question 6For an ethanol-chloroform mixture at 545 mmHg, determine: a) The Liquid - Vapor equilibrium diagram (1pt) b) Boiling temperature with 20% mass of ethanol (1pt) c) The composition of a mixture that has gone through two distillation stages (1pt)
- What is AG for the decomposition of CaCO3 at 298 K and a partial pressure of CO2 of 4.00x10-4 bar? CaCO3(s) → CaO(s) + CO2(g) AGrxn (298 K, Pco2 = 0.400 mbar) = ??? CO2(g) Compound AG°; (kJ mol·1) CACO3(s) СаО(s) -1129 -604 -394Hydrogen sulphide 8-h average limit is 20 ppm at 25°C and 1 atm. Calculate concentration of hydrogen sulphide in mg/m at 15°C and 754 mm Hg. Q.3At high altitudes, mountain climbers are unable to absorb a sufficient amount of O2 into their bloodstreams to maintain a high activity level. At a pressure of 1.00 bar, blood is typically 95.0% saturated with O2, but near 0 feet where the pressure is 0.660 bar, the corresponding degree of saturation is 60.0%. Air contains 20.99% O2 by volume. Assume that the density of blood is 998 kg m -3 Part A Assuming that the Henry's law constant for blood is the same as for water (4.95 x 104 bar), calculate the amount of O₂ dissolved in 1.00 L of blood for pressure of 1.00 bar. Express your answer with the appropriate units. mass O₂ = 3.32 μA Part B mg Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining ? Assuming that the Henry's law constant for blood is the same as for water (4.95 × 10 bar), calculate the amount of O₂ dissolved in 1.00 L of blood for pressure of 0.660 bar Express your answer with the appropriate units.