Zn(s) + 2Ag^+ (aq) rightarrow Zn^2+ (aq) + 2Ag(s) An excess of zinc metal is add
ID: 1066912 • Letter: Z
Question
Zn(s) + 2Ag^+ (aq) rightarrow Zn^2+ (aq) + 2Ag(s) An excess of zinc metal is added to 50.0 mL of a 0.100 M AgNOI_3 solution in a constant-pressure calorimeter. As a result of the reaction shown above, the temperature rises from 19.25 degree C to 22.17 degree C. The heat capacity of the calorimeter is 98.6 J/degree C. Assume that the density and specific heat of the solution are the same as those for water (which is density = 1.00g/mL and specific heat capacity = 4.184 J/g degree C), and ignore the specific heats of the metals. Calculate the amount of the heat absorbed by the solution. State your final answer using three sigfigs. Calculate the amount of the heat absorbed by the calorimeter. State your final answer using three sigfigs. Calculate the enthalpy change for the above reaction on a molar basis (meaning the final answer should be kJ per mole of Zn(s). State your final answer using three sigfigs.Explanation / Answer
a) mass of solution = d*v = 1*50 = 50 g
specificheat of solution = 4.184 j/g.c
DT = 22.17 - 19.25 = 2.92 c
heat capacity of caloremeter(C) = 98.6 j/c
heat released(q) = C*DT + msDT
= 98.6*2.92+50*4.184*2.92
= 898.78 joule
= 0.899 kj
b) heat absorbed by calorimeter = C*DT = 98.6*2.92 = 287.9 joule
= 0.288 kj
c) no of mole of Zn reacted = 2*no of mole of Ag+
no of mole of Ag+ taken = 50/1000*0.1 = 0.005 mole
no of mole of Zn reacted = 2*0.005 = 0.01 mole
DHrxn = q/n = 0.899/0.01 = 89.9 kj/mol
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