If 15.0 mL of a 1.5M HCl solution at 22.5 degrees C is mixed with 25.0mL of a 1.5M NaOH solution at 21.5 degrees C that is in a calorimeter, and the final mixed solution temperature ends up at 28.5 degrees C,

1.)what is the balanced equation for this reaction?
2.) what is the source of the heat that is causing the increase in temperature?
3.) Calculate the amount of heat absorbed or lost for the HCl/NaOH solution. Assume aqueous conditions.(Cwater=4.18J/gxK, d=1.0g/mL)
4.) Calculate the amount of het absorbed or lost by the calorimeter. The calorimeter's initial temperature is the same as the solution that is initially inside it.
5.) Determine the amount of heat absorbed or lost during this reaction.
6.)Which of the reactants is the limiting reagent? Determine the moles.
7.)Determine the amount of heat given off per mole of LR. Make sure to include an appropriate sign indicating whether it is an exothermic or endothermic process. Answer in kJ/mol

Changing screen names won't help. Read over your post carefully and make sure you have included everything. With no data to calculate it and no calorimeter constant given, 4,5,6, et al are dead in the water..

1.) To determine the balanced equation for the reaction between HCl and NaOH, we first need to write the chemical formulas for each compound.

The chemical formula for hydrochloric acid is HCl, and for sodium hydroxide, it is NaOH.

When these two compounds react, they form water (H2O) and sodium chloride (NaCl).

The balanced equation is:

HCl + NaOH -> H2O + NaCl

2.) The source of heat that is causing the increase in temperature is the exothermic nature of the reaction between HCl and NaOH. Exothermic reactions release heat, which is then absorbed by the surrounding solution and the calorimeter.

3.) To calculate the amount of heat absorbed or lost for the HCl/NaOH solution, we need to use the equation:

q = m * c * ΔT

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

First, we need to calculate the mass of the solution. Since the density (d) of water is 1.0 g/mL, the mass can be calculated as the sum of the volumes multiplied by the density:

Mass of HCl solution = 15.0 mL * 1.0 g/mL = 15.0 g
Mass of NaOH solution = 25.0 mL * 1.0 g/mL = 25.0 g

Next, we calculate the heat absorbed or lost by the solution:

q = (15.0 g + 25.0 g) * 4.18 J/gxK * (28.5°C - 22.5°C)

4.) To calculate the amount of heat absorbed or lost by the calorimeter, we use the same equation as before:

q = m * c * ΔT

The mass of the calorimeter is typically given in the question or can be determined experimentally. Let's assume it is 50.0 g, and the initial temperature (T1) of the calorimeter is 22.5°C.

q = 50.0 g * 4.18 J/gxK * (28.5°C - 22.5°C)

5.) To determine the total amount of heat absorbed or lost during this reaction, we need to sum up the heat absorbed or lost by the solution and the calorimeter:

Total heat absorbed or lost = heat absorbed or lost by solution + heat absorbed or lost by calorimeter

6.) To determine the limiting reagent, we compare the number of moles of each reactant to the stoichiometry of the balanced equation.

First, we calculate the number of moles for HCl:

Molar mass of HCl = 1 g/mol + 35.5 g/mol = 36.5 g/mol

Number of moles of HCl = Mass of HCl / Molar mass of HCl

Next, we do the same for NaOH:

Molar mass of NaOH = 23 g/mol + 16 g/mol + 1 g/mol = 40 g/mol

Number of moles of NaOH = Mass of NaOH / Molar mass of NaOH

The reactant that has fewer moles is the limiting reagent because it will be completely consumed in the reaction.

7.) To determine the amount of heat given off per mole of the limiting reagent, we divide the amount of heat absorbed or lost for the limiting reagent by the number of moles of the limiting reagent:

Heat per mole of the limiting reagent = (Heat absorbed or lost by limiting reagent / Number of moles of the limiting reagent) / 1000

The division by 1000 is done to convert from J to kJ. The sign indicating whether it is an exothermic or endothermic process can be determined by comparing the sign of the calculated value. If it is negative, it indicates an exothermic process (heat given off), and if it is positive, it indicates an endothermic process (heat absorbed).