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CHEM EXAM 3 Notecard

CHEM EXAM 3 Notecard - Small K< 1 reactants...

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Ideal Gas Law PV = nRT (P +(a*n 2 )/V 2 )(V – n*b) = nRT Percent Composition percentage by mass = mass of part/ mass of whole Next we divide the moles to try to get an even ratio. and and thus: where: P = absolute gas pressure V = gas volume n = number of moles R = universal ideal gas law constant T = absolute gas temperature ρ = gas density at T and P m = mass of gas M = molar mass of gas Formula Description Example Polar AB Linear CO HA x Single H HCl A x OH OH at 1 end C 2 H 5 OH O x A y O at 1 end H 2 O N x A y N at 1 end NH 3 Non- polar A x All elements O 2 C x A y Carbon compounds CO 2 Non-polar covalent bond: 0.0-0.4 Slightly polar bond: 0.5-0.9 Moderately polar bond: 1-1.3 Highly polar bond: 1.4-1.7 Slightly ionic bond: 1.8-2.2 Ionic Bond: 2.3+ simple body-centered face-centered Large K > 1 products are "favored" K = 1 neither reactants nor products are favored
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Unformatted text preview: Small K < 1 reactants are "favored" The value for K is large when products dominate the mixture. The value for K is small when the reactants dominate the mixture. The expression for an equilibrium reaction is determined by the coefficients in the balanced equation. added reactants cause an increase in the amount of products. Raising the temperature for an exothermic reaction favors reactants. Raising the temperature for an endothermic reaction favors formation of products. Increasing the pressure favors the side with lass volume. Increasing the concentration of a substance in the equilibrium mixture creates a temporary increase the reaction rate on that side of the equilibrium. 2 H 2 (g)+N 2 (g) N 2 H 4 (g)...
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