When 60 mL of 1.30 mol/L AgNO3(aq) and 60 mL of 1.30 mol/L HCl(aq) are mixed in a simple calorimeter, the temperature rises by 5.18°C. The molar enthalpy of reaction of HCl(aq) is ab. C kJ/mol.

Answer : The molar enthalpy of reaction is, 33.3 KJ/mole

Explanation :

First we have to calculate the mass of water.

As we know that the density of water is 1 g/ml. So, the mass of water will be:

The volume of water =

Now we have to calculate the heat absorbed during the reaction.

where,

q = heat absorbed = ?

= specific heat of water =

m = mass of water = 120 g

= change in temperature =

Now put all the given values in the above formula, we get:

Now we have to calculate the molar enthalpy of reaction.

where,

= enthalpy of neutralization = ?

q = heat released = 2.60 KJ

n = number of moles =

Therefore, the molar enthalpy of reaction is, 33.3 KJ/mole

explanation:

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- lead + phosphoric acid = hydrogen + lead(ii) phosphate