When 50.0 ml of 0.100 m agno3 is mixed with 50.0 ml of 0.100 m hcl in a coffee cup calorimeter, the temperature increases from 23.40 °c to 24.21°c. if the specific heat of the solution is 4.184 j/°c·g and its density is 1.00 g/ml, assuming that the calorimeter undergoes no heat change, calculate the enthalpy change for the following reaction in units of kj/mol agno3: agno3(aq) + hcl(aq) à agcl(s) + hno3(aq)

The enthalpy change during the reaction is -67.78 kJ/mol.

Explanation:

Volume of solution = 50.0 mL + 50.0 mL = 100.0 mL

Density of the solution = 1.00g/mL

Mass of the solution , m= 100.0 mL × 1.00 g/mL = 100 g

First we have to calculate the heat gained by the solution .

where,

q = heat gained = ?

c = specific heat of solution =

= final temperature =

= initial temperature =

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

Now we have to calculate the enthalpy change during the reaction.

where,

= enthalpy change = ?

q = heat gained = 338.904 J

Molarity of silver nitrate = 0.100 M

Volume of silver nitrate = 50.0 mL = 0.050 L

Moles of silver nitrate = n

(1 kJ= 1000 J)

Therefore, the enthalpy change during the reaction is -67.78 kJ/mol.

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"