Consider the following reaction :Ag^(+ ) (aq)+Cl^(-)(aq) rarrAgCl(s) When 10.0mLof 1.0 MAgNO_(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 specificheatof the aqueous mixture is 4.18 J //g//^(@)C, thatthe density of the mixture is 1.0 g mL^(-1) and that the calorimeter itself absorbsa negligible amountofheat, calculate the value of enthalpy change accompanying the processin kJ mol^(-1) ofAgCl.

Consider the following reaction :Ag^(+ ) (aq)+Cl^(-)(aq) rarrAgCl(s)

1.	Consider the following reaction :Ag^(+ ) (aq)+Cl^(-)(aq) rarrAgCl(s) When 10.0mLof 1.0 MAgNO_(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 specificheatof the aqueous mixture is 4.18 J //g//^(@)C, thatthe density of the mixture is 1.0 g mL^(-1) and that the calorimeter itself absorbsa negligible amountofheat, calculate the value of enthalpy change accompanying the processin kJ mol^(-1) ofAgCl.
Answer» Solution :Mass of the mixture solution`=`VOLUME `xx` Density `= 20 mL xx1 g mL^(-1) =20g` Riseis temperature`= 32.6 -25 = 7.6^(@)C` Heat evolved `= m xxC xx Delta t = 20xx 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)`