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Class 9Class 10First YearSecond Year
$When 2.00 \mathrm{~mol} of \mathrm{H}_{2} and 1.00 \mathrm{~mol} \mathrm{of} \mathrm{} \mathrm{O}_{2} at 100^{\circ} \mathrm{C} and 1 torr pressure react to produce 2.00 \mathrm{~mol} of gaseous water 484.5 \mathrm{~kJ} of energy are evolved. What are the values of (a) \Delta \mathrm{H} (b) \Delta \mathrm{E} for the production of one mole of \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) ?$

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

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

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

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

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

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