When 22.7mL of o.500 M H2SO4 is added to 22.7mL of 1.00 M KOH in a coffee-cup calorimeter at 23.50 degrees Celsius, the temperature rises to 30.17 degrees Celsius. Calculate the delta h of this reaction. (Assume that the total volume is the sum of individual volumes and that the density and specific heat capacity of the solution are the same as for pure water.) (d for water = 1.00 g/mL; c for water = 4.184 J/g x degrees Celsius.)

H2SO4 + 2KOH ==> 2H2O + K2SO4

millimoles H2SO4 = mL x M = 22.8 x 0.5 = approximately 11 (but that's an estimate).
millimoles KOH = 22.7 x 1.00 M = 22.7 mmols KOH.

q = delta H = mass H2O x specific heat x (Tfinal-Tinitial)
volume = 22.7 + 22.7 = 45.4 mL; use density to convert to grams.
q = grams x specific heat x delta T.
That gives you dH for the reaction.

To calculate the ΔH (enthalpy change) of this reaction, we need to determine the energy transferred to the solution, which can be found using the equation:

q = mcΔT

where:
q = heat transferred (in joules)
m = mass of the solution (in grams)
c = specific heat capacity of the solution (in J/g x °C)
ΔT = change in temperature (in °C)

First, let's determine the mass of the solution. Since the total volume is the sum of the individual volumes, we have:

Total volume = 22.7 mL + 22.7 mL = 45.4 mL

Since the density of water is 1.00 g/mL, the mass of the solution is:

mass = volume x density
mass = 45.4 g

Next, we need to determine the specific heat capacity of the solution. Given that the specific heat capacity of water is 4.184 J/g x °C, we can assume that the solution has the same specific heat capacity. Therefore, c = 4.184 J/g x °C.

Finally, we can determine the change in temperature:

ΔT = T final - T initial
ΔT = 30.17 °C - 23.50 °C
ΔT = 6.67 °C

Now we can calculate the heat transferred:

q = mcΔT
q = 45.4 g x 4.184 J/g x °C x 6.67 °C
q = 1266.92 J

Since the reaction involves 22.7 mL of 0.500 M H2SO4 and 22.7 mL of 1.00 M KOH, they are present in equal amounts. Therefore, the reaction is a 1:1 mole ratio.

Now we need to calculate the moles of H2SO4 reacted:

moles H2SO4 = volume H2SO4 x concentration H2SO4
moles H2SO4 = 0.0227 L x 0.500 mol/L
moles H2SO4 = 0.01135 mol

Using the mole ratio, the moles of KOH reacted will also be 0.01135 mol.

Therefore, the ΔH of the reaction can be calculated as follows:

ΔH = q ÷ moles reacted
ΔH = 1266.92 J ÷ 0.01135 mol
ΔH = 111569.26 J/mol

Hence, the ΔH of the reaction is approximately 111,569.26 J/mol or 111.57 kJ/mol.

To calculate the ΔH (enthalpy change) of the reaction, you need to use the equation:

ΔH = q/n

Where:
- ΔH is the enthalpy change (in J/mol)
- q is the heat transferred (in J)
- n is the number of moles of the limiting reactant

First, let's calculate the heat transferred (q) using the equation:

q = m * c * ΔT

Where:
- q is the heat transferred (in J)
- m is the mass of the solution (in g)
- c is the specific heat capacity of water (in J/g°C)
- ΔT is the change in temperature (in °C)

Since we are assuming the density and specific heat capacity of the solution are the same as for pure water, we can consider the mass of the solution to be the sum of the masses of H2SO4 and KOH used.

The mass of H2SO4 (sulfuric acid) can be calculated using the formula:

mass = volume * density

Given that the density of water is 1.00 g/mL and the volume is given as 22.7 mL, we can calculate the mass of H2SO4.

mass of H2SO4 = volume of H2SO4 * density of water

Next, calculate the mass of KOH (potassium hydroxide) in the same manner.

mass of KOH = volume of KOH * density of water

Now that we have the masses of H2SO4 and KOH, we can calculate the total mass of the solution.

mass of solution = mass of H2SO4 + mass of KOH

Next, we need to calculate the change in temperature (ΔT). It is given in the problem as 30.17°C - 23.50°C.

Once you have calculated the mass of the solution and the change in temperature, you can substitute these values into the equation:

q = mass of solution * specific heat capacity of water * ΔT

Finally, to calculate the ΔH, we need to determine the number of moles of the limiting reactant used in the reaction. Since both H2SO4 and KOH have a 1:1 mole ratio, we can use the volume and molarity to calculate the number of moles of H2SO4. The number of moles (n) is calculated using the formula:

moles = volume * concentration

Since the volume and concentration of H2SO4 are provided in the problem, you can calculate the moles of H2SO4.

Now, you can substitute the calculated values for mass, specific heat capacity, ΔT, and moles into the equation:

ΔH = q/n

Solve for ΔH to get the enthalpy change of the reaction.