in a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M of HCl are mixed to yield the following reaction:

Ag+ (aq) + Cl- (aq) >> AgCl (s)

the two solutions were initially at 22.60 degree celsius, and the final temperature is 23.40 degree celsius. calculate the heat the accompanies this reaction in kJ/mol of AgCl formed. assume that the combined solution has a mass of 100.0 g and a specific heat capacity of 4.18 J/(celsius)(Grams).

To calculate the heat associated with the reaction in kJ/mol of AgCl formed, you can use the formula:

q = mcΔT

Where:
q = heat (in Joules)
m = mass of the solution (in grams)
c = specific heat capacity of the solution (in J/(°C·g))
ΔT = change in temperature (in °C)

First, let's calculate the mass of the solution. Since the combined volume of the AgNO3 and HCl solutions is 100.0 mL, and their density is assumed to be approximately 1 g/mL, the mass is:

mass = volume * density
mass = 100.0 g

Next, calculate the change in temperature:

ΔT = final temperature - initial temperature
ΔT = 23.4 °C - 22.6 °C
ΔT = 0.8 °C

Now, to calculate the heat released or absorbed by the reaction, multiply the mass, specific heat capacity, and change in temperature:

q = mcΔT
q = (100.0 g)(4.18 J/(°C·g))(0.8 °C)
q = 334.4 J

Finally, convert the heat from Joules to kilojoules and calculate the heat per mole of AgCl formed. The molar mass of AgCl is 143.32 g/mol.

Heat per mole of AgCl = (334.4 J) / (1000 J/kJ) / (0.1 mol)
Heat per mole of AgCl = 3.344 kJ / 0.1 mol
Heat per mole of AgCl = 33.44 kJ/mol

Therefore, the heat that accompanies this reaction is 33.44 kJ/mol of AgCl formed.

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