When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the netionic equation below. The initial temperature of both solutions is 23.0°C. Assuming that the reaction goes tocompletion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙°C), calculatethe final temperature of the solution. Ca2+(aq) + 2 F-(aq) → CaF2(s)∆H°=-11.5 kJ

23.55°C

Explanation:

Based on the equation:

Ca²⁺(aq) + 2F⁻(aq) → CaF₂(s) ∆H°=-11.5 kJ

When 1 mole of Ca²⁺ and 2 of F⁻ reacts, 11.5kJ are released.

Thus, we need to find moles of reaction to find the heat released and using:

C = SₓmₓΔT

We can find the final temperature as follows:

Moles of reaction:

0.0500L * (0.400mol / L) = 0.0200moles Ca²⁺ = Moles of reaction

Heat produced is:

0.0200 moles * (11.5kJ / mol) = 0.23kJ

Using:

C = SₓmₓΔT

Where C is heat = 230J

S is specific heat = 4.18J/g

m is mass of solution = 100.00g

And ΔT is change in temperature

230J = 4.18J/gₓ100.00gₓΔT

ΔT = 0.55°C

As initial temperature is 23.0°C

Final temperature = 23.0°C + 0.55°C =

a

explanation:

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.