A 150.0 mL sample of a 1.50 M solution of CuSO4

is mixed with a 150.0 mL sample of 3.00 M
KOH in a coffee cup calorimeter. The temperature of both solutions and the calorimeter was
25.2°C before mixing and 31.3°C after mixing. The heat capacity of the calorimeter is 24.2 J/K.
Calculate the ΔHrxn for this reaction in units of kJ / mol of copper (II) hydroxide (19 points). Assume
the solutions is dilute enough that the specific heat and density of the solution is the same as that
of water (

CuSO4 + 2KOH ==> Cu(OH)2 + K2SO4

You have 150 x 1.50 = 225 millimols CuSO4
and 450 mmols KOH
q = mass solution x specific heat x (Tfinal-Tinitia)
I would use 300 mL = 300 g for mass soln.
Specific heat H2O is 4.184 J/g*C
Tfinal and Tinitial are given.
q is Joules/225 mmols. Convert to kJ/mol

34J

To calculate the ΔHrxn for the reaction, we need to use the equation:

ΔHrxn = qrxn / n

where:
- ΔHrxn is the enthalpy change of the reaction in kJ/mol
- qrxn is the heat released or absorbed by the reaction in J
- n is the number of moles of the limiting reactant

1. Calculate the heat released or absorbed by the reaction (qrxn):

qrxn = qsol1 + qsol2 + qcal

where:
- qsol1 is the heat released or absorbed by solution 1 (CuSO4)
- qsol2 is the heat released or absorbed by solution 2 (KOH)
- qcal is the heat absorbed by the calorimeter

2. Calculate the moles of CuSO4 and KOH using the volume and molarity of each solution:

moles_CuSO4 = volume_CuSO4 * molarity_CuSO4
moles_KOH = volume_KOH * molarity_KOH

3. Determine the limiting reactant. The reactant that produces the fewer moles of product is the limiting reactant.

4. Calculate the heat released or absorbed by the solutions, qsol1 and qsol2:

qsol1 = moles_CuSO4 * ΔHf_CuSO4
qsol2 = moles_KOH * ΔHf_KOH

where:
- ΔHf_CuSO4 is the enthalpy of formation of CuSO4
- ΔHf_KOH is the enthalpy of formation of KOH

5. Calculate the heat absorbed by the calorimeter, qcal:

qcal = Ccal * ΔT
where:
- Ccal is the heat capacity of the calorimeter
- ΔT is the change in temperature (final temperature - initial temperature)

6. Calculate the total heat released or absorbed by the reaction, qrxn:

qrxn = qsol1 + qsol2 + qcal

7. Calculate the moles of copper (II) hydroxide (Cu(OH)2) formed, taking into account the stoichiometry of the reaction.

8. Calculate the ΔHrxn:

ΔHrxn = qrxn / moles_Cu(OH)2

Let's now perform the calculations step by step:

Step 1:
ΔHrxn = qrxn / n

Step 2:
moles_CuSO4 = (150.0 mL / 1000) * 1.50 M
moles_KOH = (150.0 mL / 1000) * 3.00 M

Step 3:
Determine the limiting reactant.

Step 4:
qsol1 = moles_CuSO4 * ΔHf_CuSO4
qsol2 = moles_KOH * ΔHf_KOH

Step 5:
qcal = 24.2 J/K * (31.3°C - 25.2°C)

Step 6:
qrxn = qsol1 + qsol2 + qcal

Step 7:
Calculate the moles of Cu(OH)2 formed using the stoichiometry of the balanced equation.

Step 8:
ΔHrxn = qrxn / moles_Cu(OH)2

Please provide the enthalpy of formation values for CuSO4 and KOH so we can continue with the calculations.

To calculate the enthalpy change (ΔHrxn) for the reaction, we need to use the equation:

ΔHrxn = q / n

where q is the heat absorbed or released by the reaction and n is the amount of substance reacting.

First, let's calculate the heat absorbed or released by the reaction (q).

The heat absorbed or released in the reaction can be determined using the equation:

q = mcΔT

where q is the heat absorbed or released, m is the mass of the solution, c is the specific heat capacity of water, and ΔT is the change in temperature.

As given in the question, the heat capacity of the calorimeter is 24.2 J/K.

Since the specific heat and density of the solution are assumed to be the same as that of water, we can use the specific heat capacity of water, which is 4.18 J/g·°C.

To calculate the mass of the solution, we need to convert the volume given (150.0 mL) into grams using the density of water, which is 1.00 g/mL.

Therefore, the mass of the solution is:

mass = volume × density
mass = 150.0 mL × 1.00 g/mL = 150.0 g

Now we can calculate the heat absorbed or released (q):

q = mcΔT
q = (150.0 g + 150.0 g) × 4.18 J/g·°C × (31.3°C - 25.2°C)

Next, let's calculate the amount of substance reacting (n) in moles.

To find the amount of substance reacting, we need to determine the limiting reactant.

From the balanced chemical equation for the reaction:

CuSO4 + 2 KOH -> Cu(OH)2 + K2SO4

We can see that the stoichiometric ratio between CuSO4 and Cu(OH)2 is 1:1. This means that 1 mole of CuSO4 will produce 1 mole of Cu(OH)2.

Since the concentration of CuSO4 is 1.50 M and the volume of the CuSO4 solution is 150.0 mL, we can calculate the moles of CuSO4:

moles of CuSO4 = concentration × volume
moles of CuSO4 = 1.50 mol/L × 0.150 L = 0.225 mol

Therefore, the amount of substance reacting (n) is 0.225 mol.

Now we can calculate the enthalpy change (ΔHrxn):

ΔHrxn = q / n

Plug in the values:

ΔHrxn = q / 0.225 mol

Finally, divide the result by 1000 to convert from Joules to kilojoules (kJ):

ΔHrxn = (q / 0.225 mol) / 1000

And that's how you calculate the ΔHrxn for this reaction in units of kJ/mol of copper (II) hydroxide.