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##### Q.13 50 \mathrm{~cm}^{3} of 1.0 \mathrm{MHCl} is mixed with 50 \mathrm{~cm}^{3} of 1.00 \mathrm{M} \mathrm{NaOH} in a glass calorimeter. The temperature of the resultant mixture increases from 21.0^{\circ} \mathrm{C} to 27.5^{\circ} \mathrm{C} . Assume that calorimeter losses of heat are negligible. Calculate the enthalpy change mole-1 for the reactions. The density of solution to be considered is 1 \mathrm{gcm}^{-3} and specific heat is 4.18 \mathrm{Jg}^{-1} \mathrm{~K}^{-1} .(Ans: - 54 \mathrm{~kJ} \mathrm{~mol}^{-1} )

Q.5(a) Differentiate between the following:(i) Internal energy and enthalpy

Q.4. Define the following terms and give three examples of each(v) Exothermic reaction

Q.4. Define the following terms and give three examples of each(viii) Enthalpy of the system

(b) How do you measure the heat of combustion of a substance by bomb calorimeter.

Q.4. Define the following terms and give three examples of each(ii) Surroundings

Q.20 What is the meaning of the term enthalpy of ionization? If the heat of neutralization of \mathrm{HCl} and \mathrm{NaOH} is -57.3 \mathrm{~kJ} \mathrm{~mol}^{-1} and heat of neutralization of \mathrm{CH}_{3} \mathrm{COOH} with \mathrm{NaOH} is -55.2 \mathrm{~kJ} \mathrm{~mol}^{-1} calculate the enthalpy of ionization of \mathrm{CH}_{3} \mathrm{COOH} .(Ans: 2.1 \mathrm{~kJ} \mathrm{~mol}^{-1} )