Acids, Bases, and Buffers
... The equilibrium established when a weak acid or weak base is dissolved in and reacts with water needs closer examination. On the left side of the reaction an acid donates a proton to a base. On the right side, during the reverse reaction, the molecule that accepted the proton donates it back to the ...
... The equilibrium established when a weak acid or weak base is dissolved in and reacts with water needs closer examination. On the left side of the reaction an acid donates a proton to a base. On the right side, during the reverse reaction, the molecule that accepted the proton donates it back to the ...
one
... • The mass of one mole of a substance is called a molar mass. – The molar mass of an element is the same as its atomic mass expressed in grams. – A compound’s molar mass is the sum of the atomic masses of its component elements expressed in ...
... • The mass of one mole of a substance is called a molar mass. – The molar mass of an element is the same as its atomic mass expressed in grams. – A compound’s molar mass is the sum of the atomic masses of its component elements expressed in ...
Solution
... = -4.75 x 105 J d) Calculate the equilibrium constant for this reaction at 25°C. Are products or reactants favored at equilibrium under standard conditions? Is this consistent with part (c)? Explain your answer. dG = -RT*lnK K = e-dG/RT = e-(-4.75 x 105 J/(8.31J/(K*mol)*298 K) = 1.83 x 1083, this is ...
... = -4.75 x 105 J d) Calculate the equilibrium constant for this reaction at 25°C. Are products or reactants favored at equilibrium under standard conditions? Is this consistent with part (c)? Explain your answer. dG = -RT*lnK K = e-dG/RT = e-(-4.75 x 105 J/(8.31J/(K*mol)*298 K) = 1.83 x 1083, this is ...
CHEM 211: Physical Chemistry
... Objectives: After taking this course students are expected to understand - how energy is exchanged between the system and surroundings under different conditions. - how entropy and Gibbs free energy can be used to predict the direction of the spontaneous change and estimate the position of equilibri ...
... Objectives: After taking this course students are expected to understand - how energy is exchanged between the system and surroundings under different conditions. - how entropy and Gibbs free energy can be used to predict the direction of the spontaneous change and estimate the position of equilibri ...
Erik`s Chemistry: Thermochemistry - ECHS Chemistry
... H=qp since E=qp-P V substituting gives H= E+P V where P will usually be in atmospheric pressure, and V is volume change at that pressure. C. Laws of Thermochemistry 1. The magnitude of H is directly proportional to the amount of reactant or product. -Thus H can be used as a conversion factor in a ba ...
... H=qp since E=qp-P V substituting gives H= E+P V where P will usually be in atmospheric pressure, and V is volume change at that pressure. C. Laws of Thermochemistry 1. The magnitude of H is directly proportional to the amount of reactant or product. -Thus H can be used as a conversion factor in a ba ...
Equilibrium chemistry
Equilibrium chemistry is a concerned with systems in chemical equilibrium. The unifying principle is that the free energy of a system at equilibrium is the minimum possible, so that the slope of the free energy with respect to the reaction coordinate is zero. This principle, applied to mixtures at equilibrium provides a definition of an equilibrium constant. Applications include acid-base, host-guest, metal-complex, solubility, partition, chromatography and redox equilibria.