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Order of reaction: The sum of concentration terms on which the rate of a reaction actually depends as observed experimentally is called the order of the reaction i.e. the sum of the powers or exponents to which the concentration or pressure terms are raised in order ...

Rate constant may be defined as the rate of the reaction when the concentration of each reactant is taken as unity. That is why the rate constant is also known as specific reaction rate. Characteristics of rate constant: Some important characteristics of the rate constant are as ...

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The rate of any particular reaction depends upon the following factors: 1. Nature of the reactants: Let us consider the following two reactions: 2 NO (g) + O2 (g) -------------> 2 NO2 (g) …………….. Fast 2 CO (g) + O2 (g) -------------> 2 CO2 (g) …………….. Slow These reactions appear ...

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Features of rate of reaction are given below: 1. The rate of reaction is equal to the change in concentration divided by the time interval in which that change has taken place. 2. The rate of reaction can be expressed in terms of any reactant or product. 3. As concentration of ...

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The rate of reaction can be defined as the change in the concentration of any one of the reactants or products per unit time. The rate of the reaction depends on the molar concentrations of the reactants. The rate of the reaction means the speed ...

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The reason for the difference in rates in chemical kinetics is that a reaction involves the breaking and making of bonds. Since different bonds require different amounts of energy for breaking and different amounts of energies are evolved when different kinds of new bonds are ...

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Chemical kinetics is that branch of chemistry which deals with the study of the speeds or the rates of chemical reactions, the factors affecting the rates of the reactions and the mechanism by which the reactions proceed. It concerns itself with the measurement of rates ...

According to Henderson – Hasselbalch equation: pOH = pKb + log ([salt]/ [base]) pKb = - log Kb = - log .85 x 10-5 = 4.733 Therefore, pOH = 4.733 + log (0.2 / 0.1) = 4.733 + 0.301 = 5.034 pH = 14 – pOH = 14 – 5.034 ...

Continue Comments Off on Calculate the pH of a buffer solution containing 0.2 mole of NH4Cl and 0.1 mole of NH4OH per litre. Kb for NH4OH = 1.85 x 10-5.
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