Will medal!!!
The addition of hydrochloric acid to a silver nitrate solution precipitates silver chloride according to the reaction:
AgNO3(aq)+HCl(aq)→AgCl(s)+HNO3(aq)
When you combine 70.0mL of 0.185M AgNO3 with 70.0mL of 0.185M HCl in a coffee-cup calorimeter, the temperature changes from 23.16∘C to 24.25∘C.
Calculate ΔHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and C=4.18J/g⋅∘C as the specific heat capacity.

Question

Will medal!!!
The addition of hydrochloric acid to a silver nitrate solution precipitates silver chloride according to the reaction: 
AgNO3(aq)+HCl(aq)→AgCl(s)+HNO3(aq) 
When you combine 70.0mL of 0.185M AgNO3 with 70.0mL of 0.185M HCl in a coffee-cup calorimeter, the temperature changes from 23.16∘C to 24.25∘C.
Calculate ΔHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and C=4.18J/g⋅∘C as the specific heat capacity.

jfraser · Answer

seems to me you've been given all the information you need. calculate the $\Delta$H using the information given.

jfraser · Answer

$\Delta$H values are given in kj/mol, so you need to find the $energy$ released by the reaction, using $$Q = m*C*\Delta T$$ and solving for Q. Then find the moles of reactant (either the acid or silver nitrate) by using the molarity and volume$$moles = \frac{mole}{L} * L$$and divide #1 by #2

anonymous · Answer

C = 4.18
delta T = 24.25 - 23.16 = 1.09
mol = 0.070L * 0.185M = 0.01295
m = d*v = 1.00*(0.070+0.070) = 0.14g
So, delta H = q/mol HCl = [mC(deltaT)]/mol HCl = (0.14*4.18*1.09)/(0.01295) = 49.3 kJ

Thank you so much JFraser! I got it right.