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 =

All ideal gases occupy 22.4 L/mol at STP. To determine the volume this one will occupy you need to know how many mols of CO is in 8.81g of CO. So, you should should:

1) Convert 8.81g to mols.

2) To do this you need to calculate the molar mass of CO

3) This is calculated by using the masses of each element from the periodic table (https://ptable.com/#Properties)

4) The table tells us that 1 mol of C is 12g and that 1mol of O is 16g. So, you can determine the mass of 1 mol of CO. Lets say 1mol of CO has a mass of 20g (it doesn't).

5) Once you have that you say " if 1mol = 20g, then x mols = 8.81g) and solve the ratio.

6) This will tell you how many mols of CO you have.

7) Once you know that you say "since 1 mol of an ideal gas takes up 22.4L, then how many liters will my gas takes up if i have x mols of this gas"

And voila!

HINT: I think the answer might be between 1 - 10 L. :):)