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Problem #6: A 12.0 g sample of gas occupies 19.2 L at STP. What is the molecular weight of this gas? Solution: This problem, as well as the two just above can be solved with PV = nRT. You would solve for n, the number of moles. Then you would divide the grams given by the mole calculated. 1) Use PV = nRT: (1.00 atm) (19.2 L) = (n) (0.08206) (273 K)
The following practice problems are to master to topics on the ideal gas laws: Boyle’s law, Charles’s law, and Avogadro’s Law, as well as the combined gas law equation. There are examples to work on the Dalton law of partial pressures, the Graham’s law of effusion, and gas stoichiometry.
Solution: 1) The first thing we need to do is compute the rate of effusion for each gas: unknown gas: 2.278 x 10¯ 4 mol / 95.70 s = 2.380 x 10¯ 6 mol/s argon: 1.738 x 10¯ 4 mol / 81.60 s = 2.123 x 10¯ 6 mol/s. 2) Now, we are ready to use Graham's Law.
Chemistry 20 Worksheets 10 Worksheet 2.1: Mole to Mole Stoichiometry Directions: Write balanced equations with states. Solve the problem. Assume water is available. 1. Liquid water decomposes into its elements. How many moles of hydrogen gas are produced if 0.500 mol of water is used? 2. Sulphur reacts with barium oxide.
Example #1: 2.00 L of a gas is collected at 25.0 °C and 745.0 mmHg. What is the volume at STP? Solution: 1) You have to recognize that five (of six possible) values are given in the problem and the sixth is an x. Also, remember to change the Celsius temperatures to Kelvin.
28 maj 2020 · Write a balanced molecular equation describing each of the following chemical reactions. Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas. Gaseous butane, C 4 H 10, reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor.
Exercise 1. Derive the value of the gas constant, R, where the pressure is in torr and volume is in mL. The ideal gas law is PV = nRT. Solve for R. \(\displaystyle R\;=\;\frac{PV}{nT}\) At STP: P = 760 mmHg, V = 22410. mL, n = 1 mole, T = 273.15 K
