Exothercy Of Equilibrium

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Preliminary Questions 1. Define the following terms, both in terms of the overall energy change and in terms of the energies of reactants and products: (a) Exothermic

If a reaction is exothermic, it releases energy when a reaction takes place. The overall energy change is positive as energy is released. ∆H is negative. (b) Endothermic If a reaction is endothermic, it requires energy when a reaction is to take place. The overall energy change is negative as energy is required for a reaction to take place. ∆H is positive.

2. For an exothermic process, how is the equilibrium constant affected by temperature? For an exothermic process, bonds are made. This means at higher temperatures,
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Define enthalpy H The amount of energy used by a system at a constant pressure.

Preliminary Questions
1. What is the difference between heat capacity and specific heat capacity Heat Capacity – The energy to increase the temperature of a system by one degree.

Specific Heat Capacity – Q = m c ∆T where Q = specific heat capacity, m = mass of the object that is having its temperature raised, c = the specific heat capacity of the object being heated and ∆T = the change of temperature.

2. What do you understand in terms of reaction enthalpy ∆rH? Illustrate your answer with an example. The enthalpy change of reaction is the energy change associated with a reaction under standard conditions. E.g. 1 mol dm-3, 1 atm of pressure and 293K. ∆Hr = ∑∆H Reactants - ∑∆H Products

e.g. If total enthalpy of reactants = +221.1 KJ mol-1 and total enthalpy of products = +21.1 KJ mol-1, then reaction enthalpy = +200 KJ mol-1

TERNARY PHASE DIAGRAM Preliminary Questions 1. Define degrees of freedom for multicomponent systems. The degrees of freedom of a system are the number of variables in a system that may be changed without changing the number of phases present at
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