Question

In a coffee cup calorimeter, 50.0 mL of 0.100M $AgN{O}_3$and 50.0 mL of 0.100MHCl are mixed. The following reaction occurs:

$Ag\left(aq\right)+\frac{1}{2}C{l}_2\left(aq\right)\to AgCl\left(s\right)$

If the two solutions are initially at $22.60°C$, and if the final temperature is $23.40°C$, calculate $∆H$for the reaction in $kJ/mol$of AgCl formed. Assume a mass of 100.0 g for the combined solution and a specific heat capacity of$4.18J/g°C$ .

Short answer

$∆H$for the reaction:$∆H$ is a property of thermodynamics which is the sum of system internal energy and the product of volume and pressure.

$Ag\left(aq\right)+\frac{1}{2}C{l}_2\left(aq\right)\to AgCl\left(s\right)$is - 66.9 KJ /mol .

Step-by-step solution

About coffee cup calorimeter

A coffee cup calorimeter is a constant pressure calorimeter.

To calculate  qcal

$$\begin{gathered} q_{\left(cal\right)}=100g\times 4.18J/g°C\times (23.40°C-22.60°C) \\ =334.72J \end{gathered}$$

We know that,

$q_{\left(cal\right)}=-q_{\left(reaction\right)}$

Step 3: To calculate  ∆H for the reaction

$∆H_{\left(reaction\right)}=\frac{-334.72J}{0.1Mol/L\times 0.05L}=-66944J/mol=66.9kJ/mol$