LBS 172 Exam 2 Equations

# LBS 172 Exam 2 Equations - L · atm/K · mol and T is...

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Exam 2 Equations Molality of solute ( m ) = mol solute kg solvent Mole fraction of A ( X A ) = n A n A + n B + n C + Weight % A = mass of A mass of A + mass of B + mass of C + Henry’s Law S g = k H P g where S g is the solubility of the gas, k H is a constant, and P g is the partial pressure of the gaseous solute Raoult’s Law P solvent = X solvent solvent where P° solvent is the vapor pressure of the pure solvent Mole fraction of solvent ( X solvent ) = n solvent n solvent + (n solute x i) Elevation in boiling point T BP = T F - T I = m solute x k BP x i Freezing point depression T FP = T F - T I = m solute x k FP x i

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Osmotic pressure Π = c x R x T x i where c is solute concentration in mol/L, R is the gas constant 0.0821
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Unformatted text preview: L · atm/K · mol, and T is temperature in kelvins Rate RXN = k[A] X [B] Y where aA + bB Æ cC, x is the order of the reaction with respect to A, and y is the order of the reaction with respect to B Concentration at half-life [ R ] t ½ = ½ [R] Half-life for 0 th order reaction t 1/2 = [R] /2k Half-life for a first order reaction t 1/2 = 0.693/k Decimal % remaining for first order reactions Decimal % = 0.5 X where x is the number of half-lives that have passed Half-life for second order reaction t 1/2 = [R] /k Molecular Orbital Diagram...
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## This note was uploaded on 07/25/2008 for the course LBS 172 taught by Professor Laduca during the Spring '08 term at Michigan State University.

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LBS 172 Exam 2 Equations - L · atm/K · mol and T is...

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