Exam2 - Equations: o K = oC + 273.15 o F = 1.8 (oC) + 32...

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Equations: o K = o C + 273.15 o F = 1.8 ( o C) + 32 q = m q c q T = m q c q (T f – T i ) Constants: Specific heat capacity of water: 1.00 cal cal/g K = 4.184 J/ g K Density of water: 1.00 g/mL Universal gas constant: 0.08206 atm L/mol K = 8.314 J/mol K Conversions: 1 atm = 760 torr (exact) = 760 mm Hg (exact) Solubility Rules: Soluble ionic compounds (salts) o Always soluble: any compounds containing: Group IA cations, NH 4 + , or ClO 4 ‾, NO 3 ‾, C 2 H 3 O 2 ‾ anions o Anions that are usually soluble Compounds containing Cl‾, Br‾, or I‾ are soluble unless they bond with Ag + , Pb 2+ , Cu + or Hg 2 2+ ; Compounds containing SO 4 2- are soluble unless it bonds with Ag + , Pb 2+ , Hg 2 2+ , Ca 2+ , Sr 2+ , or Ba 2+ ; Compounds containing F‾ are soluble unless they bond with Pb 2+ , Mg 2+ Ca 2+ , Sr 2+ , or Ba 2+ ; Insoluble ionic compounds (salts) o Anions that are usually insoluble Compounds containing CO 3 2- , PO 4 3- are insoluble unless they bond with group IA ions or NH 4 + ; Compounds containing S 2- are insoluble unless it bonds with group IA ions, NH 4 + or Ca 2+ ; Compounds containing OH‾ are insoluble it bonds with group IA ions, NH 4 + , Ca 2+ , Sr 2+ , or Ba 2+ .
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Choose the one alternative that best completes the statement or answers the question. 1. Determine the volume occupied by 25.0 g of hydrogen gas at 20 o C and pressure 745 torr. (a) 304 L (b) 280 L (c) 20.9 L (d) 30.4 L (e) 607 L 2. A balloon contains 0.76 mol N 2 , 0.18 mol O 2 , 0.041 mol Ar and 0.019 mol CO 2 at 739 mmHg. What is the partial pressure of N 2 ? (a) 739 mmHg (b) 562 mmHg (c) 133 mmHg (d) 30.2 mmHg (e) 14.0 mmHg 3. If the volume of gas is reduced to half while the number of moles of gas is doubled at constant temperature, the pressure of the gas (a) is halved (b) is doubles (c) is quadrupled (d) is quartered (e) remains the same 4. A 207 mL sample of gas at 0.919 atm and 25 o C has the mass of 0.311 g. What is this gas sample? (a) H 2 (b) N 2 (c) O 2 (d) F 2 (e) Ar 5. An “empty” aerosol can at 25 o C still contains gas at 1.00 atm pressure. If this “empty” can is thrown into a 475 o C fire, what is the final pressure in the heated can? (Assuming there is no gas leaking.)
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This test prep was uploaded on 04/08/2008 for the course CHEM 1307 taught by Professor Li during the Spring '08 term at Texas Tech.

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Exam2 - Equations: o K = oC + 273.15 o F = 1.8 (oC) + 32...

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