Consider the following reaction `:` `Ag^(+ ) (aq) +Cl^(-)(aq) rarrAgCl(s)`
When 10.0mLof 1.0 M`AgNO_(3)` solution is added to 10 mL of 1.0 mL NaCl solution at `25^(@)C` in a calorimeter , a white ppt. of AgCl is formed and the temperature of the aqueous mixture mixture risesto `32.6^(@)C`. Assuming that the specific heatof the aqueous mixture is `4.18 J //g//^(@)C`, that the density of the mixture is `1.0 g mL^(-1)` and that the calorimeter itself absorbs a negligible amountofheat, calculate the value of enthalpy change accompanying the processin kJ `mol^(-1)` ofAgCl.

Explanation

Mass of the mixture solution`=`Volume `xx` Density `= 20 mL xx1 g mL^(-1) =20g`
Rise is temperature `= 32.6 -25 = 7.6^(@)C`
Heat evolved `= m xxC xx Delta t = 20 xx 4.18 xx 7.6 =640J`
Moles of`Ag^(+) =( 1)/( 1000) xx 10 =10^(-2)`
`:. ` Moles ofAgCl `= 10^(-2)`
`:. ` Heat evolved per mole of AgCl ` ( 640 )/( 10^(-2)) = 64000 J mol^(-1) = 64kJ mol^(-1)`