Chemistry The Molecular Nature Of Matter And Change 9th
Chemistry The Molecular Nature Of Matter And Change 9th
9th Edition
ISBN: 9781260240214
Author: SILBERBERG
Publisher: McGraw Hill
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Chapter 17, Problem 17.1P
Interpretation Introduction

Interpretation:

The effect on equilibrium constant and concentration of reactants and products at equilibrium has to be explained, when the reaction conditions are altered to increase the rate of forward reaction.

Concept Introduction:

Le Chatelier principle states that, whenever a system at equilibrium is disturbed, the system will undergo reactions and try to cancel that effect and reattain equilibrium. Here the disturbance means change in concentration of any of the component, change in temperature, pressure or volume.

Equilibrium constant (K) is the equilibrium ratio of concentration/partial pressure of product to reactant in which the stoichiometric term raised to the power of each component’s concentration or partial pressure. It has a particular value at a particular temperature.

Consider a reaction, a moles of A gives b moles of B as follows,

a A  b B

The equilibrium constant for this reaction can be written as follows,

K = [B]eqb[A]eqa

Where,

    [A]eq= equilibrium concentration of A[B]eq = equilibrium concentration of B   a    = stoichiometric co-efficient of A   b    = stoichiometric co-efficient of A

Expert Solution & Answer
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Explanation of Solution

According to Le-Chatelier principle, whenever a system is disturbed the system will try to nullify the effect and try to reach equilibrium.  More products can be obtained when the rate of forward reaction is greater than the rate of reverse reaction. This can be achieved by increasing the concentration of reactant, removing the product from the system or changing the temperature.

If the rate of forward reaction increased due to change in concentration, either by increasing the concentration of reactant or removing the product from the system. But the overall ratio of concentration of product to reactant remains same. So, equilibrium constant will not change.

If more products are obtained due to change in temperature then, rate of both forward and backward reaction changes. So equilibrium constant also changes. K value increases due high rate of forward reaction than reverse reaction. According to the equation below, the equilibrium constant K increases since large amount of product and small less amount of reactant present in the system.

K = [Product][Reactant]

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Chapter 17 Solutions

Chemistry The Molecular Nature Of Matter And Change 9th

Ch. 17.5 - Prob. 17.6AFPCh. 17.5 - Prob. 17.6BFPCh. 17.5 - Prob. 17.7AFPCh. 17.5 - Prob. 17.7BFPCh. 17.5 - Prob. 17.8AFPCh. 17.5 - Prob. 17.8BFPCh. 17.5 - Prob. 17.9AFPCh. 17.5 - Prob. 17.9BFPCh. 17.5 - An inorganic chemist studying the reactions of...Ch. 17.5 - Prob. 17.10BFPCh. 17.6 - In a study of glass etching, a chemist examines...Ch. 17.6 - Prob. 17.11BFPCh. 17.6 - Prob. 17.12AFPCh. 17.6 - Prob. 17.12BFPCh. 17.6 - Prob. 17.13AFPCh. 17.6 - Should T be increased or decreased to yield more...Ch. 17.6 - Prob. 17.14AFPCh. 17.6 - Prob. 17.14BFPCh. 17.6 - Prob. 17.15AFPCh. 17.6 - Prob. 17.15BFPCh. 17.6 - Many metabolites are products in branched...Ch. 17 - Prob. 17.1PCh. 17 - When a chemical company employs a new reaction to...Ch. 17 - If there is no change in concentrations, why is...Ch. 17 - Prob. 17.4PCh. 17 - Prob. 17.5PCh. 17 - Prob. 17.6PCh. 17 - Prob. 17.7PCh. 17 - Prob. 17.8PCh. 17 - Prob. 17.9PCh. 17 - Does Q for the formation of 1 mol of NO from its...Ch. 17 - Does Q for the formation of 1 mol of NH3 from H2...Ch. 17 - Balance each reaction and write its reaction...Ch. 17 - Prob. 17.13PCh. 17 - Prob. 17.14PCh. 17 - Prob. 17.15PCh. 17 - Balance each of the following examples of...Ch. 17 - Balance each of the following examples of...Ch. 17 - Balance each of the following examples of...Ch. 17 - Balance each of the following examples of...Ch. 17 - Prob. 17.20PCh. 17 - Prob. 17.21PCh. 17 - Prob. 17.22PCh. 17 - Prob. 17.23PCh. 17 - Prob. 17.24PCh. 17 - Prob. 17.25PCh. 17 - When are Kc and Kp equal, and when are they not? Ch. 17 - A certain reaction at equilibrium has more moles...Ch. 17 - Prob. 17.28PCh. 17 - Determine Δngas for each of the following...Ch. 17 - Prob. 17.30PCh. 17 - Prob. 17.31PCh. 17 - Prob. 17.32PCh. 17 - Prob. 17.33PCh. 17 - Prob. 17.34PCh. 17 - The following molecular scenes depict the aqueous...Ch. 17 - At 425°C, Kp = 4.18 × 10−9 for the...Ch. 17 - At 100°C, Kp = 60.6 for the reaction 2NOBr(g) ⇌...Ch. 17 - The water-gas shift reaction plays a central role...Ch. 17 - In the 1980s, CFC-11 was one of the most heavily...Ch. 17 - For a problem involving the catalyzed reaction of...Ch. 17 - What is the basis of the approximation that avoids...Ch. 17 - Prob. 17.42PCh. 17 - Gaseous ammonia was introduced into a sealed...Ch. 17 - Prob. 17.44PCh. 17 - Prob. 17.45PCh. 17 - Prob. 17.46PCh. 17 - Prob. 17.47PCh. 17 - Prob. 17.48PCh. 17 - Prob. 17.49PCh. 17 - Prob. 17.50PCh. 17 - Nitrogen dioxide decomposes according to the...Ch. 17 - Hydrogen iodide decomposes according to the...Ch. 17 - Compound A decomposes according to the...Ch. 17 - Prob. 17.54PCh. 17 - Prob. 17.55PCh. 17 - Prob. 17.56PCh. 17 - A toxicologist studying mustard gas, S(CH2CH2Cl)2,...Ch. 17 - Prob. 17.58PCh. 17 - A key step in the extraction of iron from its ore...Ch. 17 - What does “disturbance” mean in Le Châtelier’s...Ch. 17 - Prob. 17.61PCh. 17 - Prob. 17.62PCh. 17 - Prob. 17.63PCh. 17 - Le Châtelier’s principle is related ultimately to...Ch. 17 - An equilibrium mixture of two solids and a gas, in...Ch. 17 - Consider this equilibrium system: CO(g) + Fe3O4(s)...Ch. 17 - Sodium bicarbonate undergoes thermal decomposition...Ch. 17 - Prob. 17.68PCh. 17 - Prob. 17.69PCh. 17 - Predict the effect of decreasing the container...Ch. 17 - Prob. 17.71PCh. 17 - Prob. 17.72PCh. 17 - Prob. 17.73PCh. 17 - Prob. 17.74PCh. 17 - Prob. 17.75PCh. 17 - Prob. 17.76PCh. 17 - The formation of methanol is important to the...Ch. 17 - Prob. 17.78PCh. 17 - The oxidation of SO2 is the key step in H2SO4...Ch. 17 - A mixture of 3.00 volumes of H2 and 1.00 volume of...Ch. 17 - You are a member of a research team of chemists...Ch. 17 - For the following equilibrium system, which of the...Ch. 17 - Prob. 17.83PCh. 17 - Prob. 17.84PCh. 17 - Prob. 17.85PCh. 17 - Prob. 17.86PCh. 17 - Prob. 17.87PCh. 17 - Prob. 17.88PCh. 17 - Prob. 17.89PCh. 17 - Prob. 17.90PCh. 17 - When 0.100 mol of CaCO3(s) and 0.100 mol of CaO(s)...Ch. 17 - Prob. 17.92PCh. 17 - Prob. 17.93PCh. 17 - Prob. 17.94PCh. 17 - Highly toxic disulfur decafluoride decomposes by a...Ch. 17 - A study of the water-gas shift reaction (see...Ch. 17 - Prob. 17.97PCh. 17 - Prob. 17.98PCh. 17 - Prob. 17.99PCh. 17 - Prob. 17.100PCh. 17 - Prob. 17.101PCh. 17 - Prob. 17.102PCh. 17 - The molecular scenes below depict the reaction Y ⇌...Ch. 17 - For the equilibrium H2S(g) ⇌ 2H2(g) + S2(g) Kc =...Ch. 17 - Prob. 17.105PCh. 17 - Prob. 17.106PCh. 17 - The kinetics and equilibrium of the decomposition...Ch. 17 - Isopentyl alcohol reacts with pure acetic acid to...Ch. 17 - Isomers Q (blue) and R (yellow) interconvert. They...Ch. 17 - Glauber’s salt, Na2SO4·10H2O, was used by J. R....Ch. 17 - Prob. 17.111PCh. 17 - Synthetic diamonds are made under conditions of...
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