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notes%20for%20final%20p2 - Gay-Lussac P 1 T 2 =P 2 T 1...

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General Chemistry Notes Molar Mass: Cu(NO 3 ) 2 ·2H 2 0 1 Cu + 2N + (3x2)O + 2H 2 O = 63.5+ 2x14.0 + 6x16.0 + 2x18.0 = 223.5g/mole Grams of sample divided by moles of sample = molar mass Reaction Types Decomposition AX A +X Synthesis A+X AX Oxidation 2A + O 2 2AO Double Replacement AX+BY AY + BX Single Replacement (Single Displacement) AX+B BX+A or AX + Y AY+X Activity Series lithium potassium strontium calcium sodium magnesium aluminum zinc chromium iron cadmium cobalt nickel tin lead hydrogen antimony arsenic bismuth copper mercury silver paladium platinum gold 1 atm equals 760 torr 760 mm Hg 101.3 kPa Ideal gas constant R= 0.0821 L·atm K·mol = 8.314 L·kPa K·mol = 62.3637 L·mmH g K·mol Half Lives # of Amount Half Lives Remaining 0 1 (all) 1 1/2 2 1/4 3 1/8 4 1/16 5 1/32 6 1/64 Alpha particle 2 4 He Beta Particle (electron) 1 0 e Positron 1 0 e neutron 0 1 n Common acids Sulfuric H 2 SO 4 Hydrochloric HCl Nitric HNO 3 Phosphoric H 3 PO 4 Acetic CH 3 COOH Perchloric HClO 4 Common bases Sodium Hydroxide NaOH Ammonia NH 3 Gas Laws Boyles P 1 V 1 =P 2 V 2 Charles V 1 T 2 =V 2 T 1
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Unformatted text preview: Gay-Lussac P 1 T 2 =P 2 T 1 Combined P 1 V 1 T 2 =P 2 V 2 T 1 Ideal PV=nRT Dalton P t = P 1 +P 2 +P 3 ... Common Ions +2 Hg 2 2+ mercury(I) +1 NH 4 + ammonium H 3 O + hydronium -1 C 2 H 3 O 2-acetate ClO 3-chlorate ClO 2-chlorite CN-cyanide H 2 PO 4-dihydrogen phosphate HCO 3-hydrogen carbonate or bicarbonate HSO 4-hydrogen sulfate or bisulfate OH-hydroxide ClO-hypohlorite NO 3-nitrate NO 2-nitrite ClO 4-perchlorate MnO 4-permanganate SCN-thiocyanate -2 CO 3 2-carbonate CrO 4 2-chromate Cr 2 O 7 2-dichromate HPO 4 2-hydrogen phosphate O 2 2-peroxide SO 4 2-sulfate SO 3 2-sulfite S 2 O 3 2-thiosulfate -3 PO 4 3-phosphate Examples of molecular and empirical formula Molecular Empirical C 6 H 4 O 6 C 3 H 2 O 3 CH 3 COOH CH 2 O Mass to Mass Stoichiometry Grams initial 1 mole initial Moles final (a) Molar mass final = Grams Final Molar mass initial Moles initial (a) 1 mole final (a) from balanced equation...
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This note was uploaded on 05/01/2010 for the course CHEM Chem617 taught by Professor Otto during the Spring '09 term at Algoma University.

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