Use the information in this thermochemical equation to solve the following probl

Question

Use the information in this thermochemical equation to solve the following problem. AgNO3 HCI AgcI HNO3 -68 75.0 mL of 0.840 M AgNO3 and 75.0 mL of 0.840 M HCI are mixed in a constant-pressure (coffee-cup) calorimeter. The two solutions are both initially at 20.0 degree centigrade. Predict the final temperature of the solution after the reaction. Assume that the aqueous solutions have the same specific heat as water (4.184 J g oC) and the same density of water (1.00 g/mL). 29.7°C 35.1 °C 21.1OC 14.8 oC 24.3 oC 19.6 °C 26.8 oC 31.0oC

Explanation / Answer

HRxn = -68 kJ/mol

mol of AgNO3 = MV = 0.84*75 = 63

mol of HCl = MV = 0.84*75 = 63 --> 63*10^-3 mol

expected heat

Q = n*HRxn = ( 63*10^-3 )(68) = 4.284 kJ will be released

then

Qabs = 4.284 kJ

Q = m*C*(Tf-Ti)

4.284*10^3 = (75+75)*4.184*(Tf-20)

(4.284*10^3)/((75+75)*4.184) = Tf - 20

Tf = (4.284*10^3)/((75+75)*4.184) + 20

Tf = 26.82 °C

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