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CHEM 1A Lecture Notes - Lecture 20: Reaction Quotient, Sulfur Trioxide, Exothermic Process

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9 Nov 2016

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CHEM 1A Full Course Notes

CHEM 1A Full Course Notes

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If two or more reactions are added to give another, the equilibrium constant for the reaction is the product of the equilibrium constants of the equation added. The equilibrium constant, k, is constant as long as temperature is constant. Can cause a shift in the equilibrium position can cause a change in the value of k. Heat + h2o (l) h2o (g) More h2o (g) is produced: ph2o increases. Shift in equilibrium position to the right. Exothermic: a process that releases energy in the form of heat. Endothermic: a process or reaction that absorbs energy in the form of heat. As temperature increases, k goes down which means the heat is on the. For the general reaction: aa + bb cc + dd. The reaction quotient q = [c]c[d]d / [a]a[b]b. Q gives the ratio of product concentrations to reactant concentrations at any point in a reaction. 2 no(g) n2 (g) + o2 (g) kp = 2. 4 x 103.

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Related Questions

ENT ives To determine equilibrium concentrations for species in solution . Examine temperature effects on reaction equilibrium Investigate the shift in equilibrium from different stresses on a system kills . Use colorimeter to determine unknown solution concentrations ced .Preparing temperature baths to change reaction conditions tionEquilibrium is defined as a state in which the concentrations of both the reactants and products have no tendency to change with time. We can restate this by saying that the rate of the forward reaction is equal to the rate of the reverse reaction. Recall that with rate we are simply defining how fast a reaction is proceeding, a speed at which the reaction proceeds. Take note that when writing an equilibrium expression, pure liquids (denoted by l or 2) and pure solids (denoted by s) are omitted. Typically we express the equilibrium by K or Kp where c and p denote either concentration or partial pressure respectively. We refer to this value of K, or Kp as an equilibrium constant For any reaction, Kc can be written as the product of the concentration of products, raised to their stoichiometric coefficients, divided by the product of the concentration of the reactants raised to their stoichiometric coefficients. See Equation (5-1) below for an example: aA(aq) + bB(aq-cC(aq) + dD(aq) (5-1) A] [B]b As mentioned before, K, or K, are equilibrium constants meaning that they will have the same value unless temperature is changed. This brings in two important ideas 1) We can perturb the equilibrium concentrations of a reaction, say [A] for instance which will cause the other concentrations to shift so that K for the reaction remains constant. 2) If we change temperature, we will either increase or decrease our value of K depending on the specific reaction we are examining. Determining K, and Equilibrium Concentrations During lecture we often discuss the idea of using ICE tables as a method for organizing and calculating concentrations of reactions as they proceed towards equilibrium. In a typical ICE table you need to know initial concentrations and the magnitude of K to determine the equilibrium concentrations. Alternatively, if you know the equilibrium concentrations for a reaction you can calculate K. For this experiment we will be examining a complex ion formation, when iron(III) ion

Which of the following actions will cause the equilibrium to shift such that the concentration of NOgas will increase?

2NO(g) + 2H2(g) ? N2(g)+2H2O+heat

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Which of the following actions will cause the equilibrium to shift such that the concentration of gas will increase?

Decrease the concentration of N2(g)

Increase the concentration of H2O(g)

Increase the concentration of H2(g)

Lower the reaction temperature

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Part B

Which equilibrium reaction will experience a shift towards the products in equilibrium position when the concentration of Ni2+ is increased?

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Which equilibrium reaction will experience a shift towards the products in equilibrium position when the concentration of is increased?

NiS(s)?Ni2+(aq)+S2?(aq)

[Ni(H2O)6]2+(aq)+3en(aq)?[Ni(en)3]2+(aq)+6NH3(aq)

Ni(OH)2(s)?Ni2+(aq)+2OH?(aq)

Ni2+(aq)+6NH3(aq)?[Ni(NH3)6]2+

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Part C

When this reaction in equilibrium is heated, a red/brown color persists. What is true about this reaction?

2NO2(g)brown/red?N2O4(g)colorless

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When this reaction in equilibrium is heated, a red/brown color persists. What is true about this reaction?

The reaction is exothermic.

?H for this reaction is positive.

Heat acts as a reactant in this equilibrium.

The increase in T results in a high K value.

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