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Chapter 17: Q40P (page 776)

(a) What is the basis of the approximation that avoids using the quadratic formula to find an equilibrium concentration?

(b) When should this approximation not be made?

Short Answer

Expert verified
  1. When K is small, and the initial concentration is big, the approximation applies when the shift in concentration from initial to equilibrium concentration is so comparable that it is inconsequential.
  2. When the change in concentration is higher than 5%, the approximation should not be employed. This can happen when very tiny or when [reactant] changes dramatically due to a big K.

Step by step solution

01

Step 1: (a) What is the basis of the approximation?

When performing chemical calculations, we are usually concerned with employing the most precise data and formulae to arrive at a satisfactory result. However, there are situations whenapproximations are warranted to make computations easier or even practicable.

Theapproximationapplies when the change in concentration from initial to equilibrium concentration is so similar that it is insignificant. This occurs when K is small, and the initial concentration is large.

02

(b) When should this approximation not be made?

The approximation should not be used when the change in concentration is greater than 5%. This can occur when Reachantinitialis very small or when the change in is relatively large due to large K.

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Most popular questions from this chapter

For a given reaction at a given temperature, the value of K is constant. Is the value of Q also constant? Explain.

Consider the following reaction:

3Fe(s)+4H2O(g)鈬�Fe3O4(s)+4H2(g)

(a) What is the apparent oxidation state ofFe in Fe3O4 ?

(b) Actually, Fe has two oxidation states in Fe3O4. What are they?

(c) At 900掳C,Kcfor the reaction is 5.1. If 0.050molofH2O(g) and 0.100mol ofFe(s) are placed in a1.0鈭�L container at900掳C , how many grams of Fe3O4 are present at equilibrium?

Note: The synthesis of ammonia is a major process throughout the industrialized world. Problems 17.99 to 17.105 refer to various aspects of this all-important reaction:

N2(g)+3H2(g)鈬�2NH3(g)鈥夆赌夆赌�螖贬rxn掳=鈭�91.8kJ

You are a member of a research team of chemists discussing the plans to operate an ammonia processing plant: N2(g)+3H2(g)2NH3(g)

(a) The plant operates at close to 700 K, at which Kpis role="math" localid="1654929481926" 1.00脳10-4, and employs the stoichiometric 1/3 ratio of N2/H2. At equilibrium, the partial pressure of NH3is 50atm. Calculate the partial pressures of each reactant and Ptotal.

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For the reaction M2+N2鈬�2MN, scene A represents the mixture at equilibrium, with Mblack and Norange. If each molecule represents0.10mol and the volume is localid="1656945725597" 1.0L , how many moles of each substance will be present in scene B when that mixture reaches equilibrium?

Predict the effect of decreasing the container volume on the amounts of each reactant and product in the following reactions:

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