In an experiment, 95.0 mL of 0.225 M silver nitrate was mixed rapidly with 47.5 mL of 0.225 M calcium chloride in a coffee cup calorimeter. If a reaction occurred, was it exothermic or endothermic? If the reaction started at 23.7 °C, what is the final temperature of the solution?

dHf=-99.4 kJ/mol (AgNO3)

dHf= -795.0 kJ/mol (CaCl2)
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To determine whether the reaction is exothermic or endothermic, we need to examine the change in temperature of the solution. If the temperature increases, then the reaction is exothermic, meaning it releases heat. If the temperature decreases, then the reaction is endothermic, meaning it absorbs heat.

To find the final temperature of the solution, we can use the principle of heat capacity:

q = m * C * ΔT

Where:
q represents the heat gained or lost by the solution.
m is the total mass of the solution.
C is the specific heat capacity of the solution.
ΔT is the change in temperature of the solution.

In this case, since the reaction mixture is the same volume and concentration, we can assume that the specific heat capacity is uniform throughout the solution. Therefore, we can disregard the specific heat capacity in our calculations, giving us:

q = m * ΔT

Now we can calculate the heat gained or lost by the solution using the equation:

q(AgNO3) + q(CaCl2) + q(solution) = 0

The heat gained or lost by the reactants (silver nitrate and calcium chloride) and the heat gained or lost by the solution (the change in temperature) sum up to zero because we assume no heat is lost to the surroundings.

Since the molar ratio of AgNO3 and CaCl2 is 1:1, the amount of heat gained or lost by each is the same. Therefore:

q(AgNO3) = -q(CaCl2)

Now, let's calculate the heat gained or lost by each component using the equation:

q = m * ΔT

For silver nitrate (AgNO3):
m(AgNO3) = V(AgNO3) * ρ(AgNO3)

Where:
V(AgNO3) is the volume of silver nitrate solution (in liters)
ρ(AgNO3) is the density of silver nitrate solution (in g/mL or g/cm³)

For calcium chloride (CaCl2):
m(CaCl2) = V(CaCl2) * ρ(CaCl2)

Where:
V(CaCl2) is the volume of calcium chloride solution (in liters)
ρ(CaCl2) is the density of calcium chloride solution (in g/mL or g/cm³)

For the total mass of the solution:
m(solution) = m(AgNO3) + m(CaCl2)

Finally, to find the change in temperature ΔT, we use the equation:

ΔT = q(solution) / (m(solution) * c(solution))

Where:
c(solution) is the specific heat capacity of the solution.

By plugging in the values of the given volumes, concentrations, and density of the solutions, and assuming that the density is approximately equal to 1 g/mL, we can calculate the final temperature using the above equations.

You don't provide enough information to answer this question. Look up the delta Ho formation and provide that data.