If the number of moles of a gas are doubled at the same temperature and pressure, will the volume increase or decrease? 4. At what pressure would 0.150 mole of nitrogen gas at 23.0 °C occupy 8.90 L? 5. Find the volume of 2.40 mol of gas whose temperature is 50.0 °C and whose pressure is 202 kPa.
Fill a 10 mL graduated cylinder with ≈ 7mL if water c. Fill a 1000 mL beaker with ≈ 750 mL of water d. Invert the graduated cylinder into the beaker. Add water to the beaker to completely submerge cylinder. e. Measure the difference between the height of the water in the graduated cylinder and the height of the water in the beaker. f. g. Record the barometric pressure in mmHg. Heat the water via Bunsen burner to 80°C.
Using the same formula as above, bulk whiskey would become 5,030,000 / .52 * 1.15 = $11,124,038.46 and finished whiskey would become 1,969,000 / 11.20 *12.10 = $2,127,223.21. This leads to a total increase in inventories of
By Graham's Law (see the answer to question #1), we have: 1 / 50 = √(2.02 / x) x = 5050 g/mol Video: Solution to a Graham's Law Problem Problem #3: Two porous containers are filled with hydrogen and neon respectively. Under identical conditions, 2/3 of the hydrogen escapes in 6 hours. How long will it take for half the neon to escape? Solution: Set rate1 = H2 = x Set rate2 = Ne = 1 The molecular weight of H2 = 2.02 The molecular weight of Ne = 20.18 By Graham's Law: x / 1 = √(20.18 / 2.02) x = 3.16 Since the H2 escapes 3.16 times as fast as Ne, this calculation determines the amount of Ne leaving in 6 hours: 0.67 / 3.16 = 0.211 Calculate the time needed for half the Ne to escape, knowing that 0.211 escapes in 6 hours: 0.211 / 6 = 0.50 / x x = 14.2 hours Problem #4: If the density of hydrogen is 0.090 g/L and its rate of diffusion is 5.93 times that of chlorine, what is the density of chlorine? Solution: Set rate1 = H2 = 5.93 Set rate2 = Cl2 = 1 The molecular weight of H2 = 2.02 The molecular weight of Cl2 = x.
Week 5 RES/ 341 Chapter Exercises: 7.54 The fracture strength of a certain type of manufactured glass is normally distributed with a mean of 579 MPa with a standard deviation of 14 MPa. (a) What is the probability that a randomly chosen sample of glass will break at less than 579 MPa? (b) More than 590 MPa? (c) Less than 600 MPa? (Data are from Science 283 [February 26, 1999], p.
The system was heated for 4-5 hr under vacuum at 200°C and then cooled down to the temperature (50°C) where we want to perform the adsorption study. Small doses of test gases consecutively introduced to the system and gradually increased up to 50 Torr until an equilibrium pressure was reached. Then the obtained differential heats of the test gases adsorption were recorded as a function of its coverage. Further, the manifold degassed under vacuum for almost 30 minutes; adsorption was conducted in the same manner. Finally, the number and strength of active surface are obtained from the difference between the adsorbed gases from the first and second
This exothermic reaction increases the temperature inside the bomb, which then transfers the energy to the external water jacket raising the external temperature. It is this rise in the water-jacket temperature which is monitored and then back-calculated to obtain energy release by the combustion reaction. 1. Construction of Bomb Calorimeter A weighed sample of substance is placed in contact with an ignition wire inside the bomb. The bomb is filled to about 20 atm of pressure with O2, sealed, and placed in a known amount of water.
5. Shake and allow for the reaction to occur. 6. Measure the diameter of the balloon at 2 minute intervals then shake the flask again to further mix the contents. Results: SUGAR YEAST 5g Yeast - 20g Sugar 4.5 cm 5g Yeast - 20g Sugar 4.5 cm 5g Yeast -
Discovery Phase solid Density(near r.t.) 4.933 g·cm−3 Melting point 386.85 K236.66 °F 113.7 °C, , Boiling point 363.7 °F 184.3 °C, 457.4 K, Triple point 386.65 K, 12.1 kPa Critical point 819 K, 11.7 MPa Iodine was discovered by French chemist Bernard Courtois in 1811. At the time of the Napoleonic Wars, France was at war and saltpeter was in great demand. Saltpeter produced from French niter beds required sodium carbonate, which could be isolated from seaweed collected on the coasts of Normandy and Brittany. To isolate the sodium carbonate, seaweed was burned and the ash washed with water. The remaining waste was destroyed by adding sulfuric acid.
Johannes Kepler was born on December 27, 1571 in Germany. He was a mathematician, astronomer, and astrologer. He was most famous for his eponymous laws of planetary motion. Based on his work on Astronomia nova, Harmonicies Mundi, and Epitome of Copernican Astronomy it provided a foundation for Issac Newton’s theory of universal gravitation. Early Life Johannes Kepler was born on December 27, 1571 which was also the same day as feast day of St. John the Evangelist.