Question

In a coffee cup calorimeter, 50.0 mL of 0.100 M AgNO_3 and 50.0 mL of 0.100 M HCl are mixed. The following reaction occurs:

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)
If the two solutions are initially at 22.60ᵒ C, and if the final temperature is 23.40ᵒ C, calculate ∆H for the reaction in kJ/mol of AgCl formed. Assume a mass of 100.0 g for the combined solution and that the specific heat capacity of the o -1 -1 solution is 4.184 J C g .

Answer 1

To calculate ΔH for the reaction Ag⁺(aq) + Cl⁻(aq) → AgCl(s), multiply the volume of the solution by the molarity to find the moles of AgCl formed. Calculate the heat absorbed or released using the equation q = m * c * ΔT. Finally, divide the heat by the moles of AgCl formed to get the enthalpy change per mole of AgCl.

Step-by-step explanation:

In a coffee cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed. The reaction that occurs is: Ag+(aq) + Cl-(aq) → AgCl(s). To calculate ΔH for the reaction in kJ/mol of AgCl formed, we can use the equation q = m * c * ΔT, where q is the heat absorbed or released, m is the mass of the solution, c is the specific heat capacity, and ΔT is the change in temperature. First, calculate the moles of AgCl formed by multiplying the volume of the solution by the molarity. Then, calculate the heat absorbed or released using the equation q = m * c * ΔT. Finally, divide the heat by the moles of AgCl formed to get the enthalpy change per mole of AgCl.