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An excess of zinc metal is added to 50.0 mL of a. 0.100 M
Chapter 6, Problem 115P(choose chapter or problem)
An excess of zinc metal is added to 50.0 mL of a 0.100 M \(\mathrm{AgNO}_{3}\) solution in a constant-pressure calorimeter like the one pictured in Figure 6.9. As a result of the reaction
\(Z n(s)+2 \mathrm{Ag}^{+}(a q) \rightarrow Z n^{2+}(a q)+2 A g(s)\)
the temperature rises from \(19.25^{\circ} \mathrm{C}\) to \(22.17^{\circ} \mathrm{C}\). If the heat capacity of the calorimeter is \(98.6\ \mathrm{J} /{ }^{\circ} \mathrm{C}\), calculate the enthalpy change for the above reaction on a molar basis. Assume that the density and specific heat of the solution are the same as those for water, and ignore the specific heats of the metals.
Questions & Answers
QUESTION:
An excess of zinc metal is added to 50.0 mL of a 0.100 M \(\mathrm{AgNO}_{3}\) solution in a constant-pressure calorimeter like the one pictured in Figure 6.9. As a result of the reaction
\(Z n(s)+2 \mathrm{Ag}^{+}(a q) \rightarrow Z n^{2+}(a q)+2 A g(s)\)
the temperature rises from \(19.25^{\circ} \mathrm{C}\) to \(22.17^{\circ} \mathrm{C}\). If the heat capacity of the calorimeter is \(98.6\ \mathrm{J} /{ }^{\circ} \mathrm{C}\), calculate the enthalpy change for the above reaction on a molar basis. Assume that the density and specific heat of the solution are the same as those for water, and ignore the specific heats of the metals.
ANSWER:Step 1 of 3
Here we have to calculate the enthalpy change for the above reaction on a molar basis.
Given:
The given chemical reaction is,
\(\mathrm{Zn}(\mathrm{s})+2 \mathrm{Ag}^{-}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\)
Volume of \(\mathrm{AgNO}_{3}=50.0 \mathrm{~mL}\)
Concentration \(=0.100 \ \mathrm{M}\)
Initial temperature \(\left(T_{1}\right)=19.25^{\circ} \mathrm{C}\)
Final temperature \(\left(\mathrm{T}_{2}\right)=22.17^{\circ} \mathrm{C}\)
Heat capacity \(\text { (C) }=98.6 \mathrm{~J} /{ }^{\circ} \mathrm{C}\)