Question on Equilibrium of Rigid Body?
Not too bright. Can’t solve this simple problem. Am missing something. Depressed. Desperate. From Halliday & Resnick, Fundamentals of Physics, Chapter on Equilibrium of Rigid Bodies, problem 7(3), page 218. (Vector sum of forces and torques each separately 0) A car is stuck in mud by the side of the road. A man attaches a rope to the bumper and then to a pole 6o feet away and applies a force of 125 lbs sideways at the midpoint of the rope displacing the center of the rope 1 foot (in the horizontal direction) and the car almost moves (remains in equilibrium – my comment). What force does the rope exert on the car. Answer: 1900 lbs. Help!
Equilibrium constant question...?
Ok, I've been doing all right so far in this chapter, but this question has totally confused me! Any help would be appriciated... Q: HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A- ? a) HA (aq) + H2O (l) <=> H2A+ (aq) = OH- (aq) b) A- (aq) + H3O+ (aq) <=> HA (aq) + H2O (l) c) HA (aq) + OH- (aq) <=> H2O (l) + H+ (aq) d) A- (aq) + H2O (l) <=> HA (aq) + OH- (aq) Thank you for your help!
Please Help with this Chemistry Equilibrium Question:?
As temperature increases, K decreases, indicating less products and more reactants (K=products/reactants). Because this is true, that means that the reaction went in the reverse direction. The reaction would go in the reverse direction to get rid of the added heat, meaning that the heat had to be added to the right side. Therefore, the reaction is exothermic because heat is released from the reaction (negative change in heat)
How can I prepare equilibrium chapter for JEE?
For chemical equilibrium, Start fromDifference between reversible and irreversible reactionsLaw of mass actionConcept of EquilibriumCharacteristics of Equilibrium constant,Relation between Kp and KcExpression of Kp and Kc in terms of degree of dissociation for different reversible reactions.Concept of reaction quotient (predicting the direction of reaction)Value of equilibrium constant (extent of reaction)Factors affecting equilibrium constantFactors affecting equilibrium and Le-chatelier principleSolve Numericals from exemplar, ncert, last year questions and reference book.For Ionic Equilibrium,Acid base theoriesConjugate acids and basesAmphiprotic speciesAutoprotolysis of water (Autoprotolysis constant and ionic product of water)Concept of pH and pH scalepH ofStrong Acids and bases and their mixturesWeak acids and bases (Ostwald dilution law)Weak acid in presence of SAWeak acid in presence of Common ion from its salt (Common ion effect)Weak acid and its titration vs strong baseBuffer solutionsSalt hydrolysisweak dibasic acidAmphiprotic saltsmixture of weak acidsacid base titration curvesSolubility of sparingly soluble salts and KspCondition of precipitationApplication in salt analysisExtra topics:Calculation of degree of dissociation from VD measurementsMutual solubilityFractional precipitation
Some chemistry questions - Acids, Bases, and acid-base equilibrium?
Hi. I'm working on a chapter review for my AP Chemistry class, on the topics of Acids, Bases, and Acid-Base Equilibrium. There are several questions that have me stumped. They are all multiple choice, which means that there should be some direction to go with the answers, but frankly, I have no idea how to approach them. Here they are: In the equilibriums shown below, which conjugate acid/base pair contains the strongest acid? H3PO4 + H2O <-> H2PO4- + H3O+; Ka = 7.5 x 10^-3 H2PO4- + H2O <-> HPO4(2-) + H 3O+; Ka = 76.2 x 10^-8 A. H3PO4/ H2PO4- B. H2O / H3O+ C. H2PO4- / HPO4(2-) D. H2PO4- / H2O E. H3PO4/ H3O+ B(OH)3 is which of the following: A. Brønsted-Lowry base only B. Brønsted-Lowry and Lewis base only C. Lewis base only D. Brønsted-Lowry acid only E. Lewis acid only (continued...)
Equilibrium Constant and Reaction Quotient?
A mixture initially contains A, B and C in the following concentrations:[A] = 0.700 ,[B] = 1.05 , and [C] = 0.500 . The following reaction occurs and equilibrium is established: A+2B = C At equilibrium,A = 0.510 and C = 0.690 . Calculate the value of the equilibrium constant, .
The value of the equilibrium constant?
The value of the equilibrium constant tells you *nothing* about the rate of a reaction. It only tells you which side of the reaction is favored, and by how much. Reactions that have large positive equilibrium constants are energetically favored to "go" in the forward direction, but can persist in a disequilibrium state for extremely long times without reacting (i.e., the reaction rates can be extremely slow). For instance, a mixture of H2 and O2 gases is energetically favored to react and form H2O, but will not do so unless "helped" by a catalyst or a spark/flame! You can say nothing in general about the effect of temperature on an equilibrium constant. It depends on the reaction. For instance, the equilibrium constant for the reaction: CaCO3(s) <-> CO2(g) + CaO(s) Keq = P_CO2 increases with increasing temperature. However, all we have to do is write the reaction in reverse: CaO(s) + CO2(g) <-> CaCO3(s) Keq = 1/P_CO2 and the equilibrium constant now decreases with increasing temperature.