CHEM 1211 Lecture 24Outline of Last Lecture I. Behaviors of GasesII. General Properties of GasIII. PressureIV. Boyle’s LawV. Charles’s LawVI. General Gas LawOutline of Current Lecture I. Avogadro’s hypothesisII. Ideal Gas LawA. RulesB. Types of problems you may encounterIII. Standard temperature and pressureIV. Gas DensityCurrent Lecture: I. Avogadro’s hypothesis2H2(g) + O2(g) 2H2O(g)8 molecules + 4 molecules = 8 molecules + =II. Ideal Gas LawP x V = constantn x TP x V = n x R x TR= gas constant = 0.08206 L x atmosphere / mol x KA. Rules1. Convert temperature to K2. Convert grams to moles3. Convert to units of R (L, atm, mol, K)B. Types of problems you may encounter1. Determine one unknown quantity of one gas variable (P, V, T, n) given the other values directly or indirectly2. Stoichiometry problems3. Determine the new values of P, V, T, or n after a gas undergoes a change.4. Gas density and molar mass problemsIII. Standard temperature and pressure1 atm. (760 torr or mm Hg and 0°C (273.15 K))PV=nRT v = nRT / P (standard molar volume of any gas) V = 1 mol (0.08206 L x atmosphere / mol x K) (273.15K) / 1.00 atmIV. Gas Density- D is directly proportional to P and Mwt- D is indirectly proportional to T- N = moles = mass (g) x 1 / Mwt (g/mol)M = P x Mwt = DensityV RT
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