Question

In a constant pressure glory meter 70 mL of 0.310 MBA parentheses OH parentheses two was added to 7 mL of 0.620 moles of HCl the reaction cause the temperature of the solution for two rise from 21.27°C to 25.49°C is the solution has the same density as specific as the water 1 g/mL and 4.184 J per gram times degrees Celsius respectively what is delta H for this reaction per mole H2O produced assume that the total volume is the sum of the individual volumes

Answer 1

The ΔH for the reaction per mole of H₂O produced is 2137.13 J/mol.

How to find enthalpy?

Calculate the heat absorbed by the solution:

Use the formula: Q = mcΔT

m = total mass of solution =

(70 mL + 7 mL) × 1 g/mL = 77 g

c = specific heat of solution = 4.184 J/g°C

ΔT = final temperature - initial temperature

= 25.49°C - 21.27°C

= 4.22°C

Therefore;

Q = 77 g × 4.184 J/g°C × 4.22°C

= 1325.02 J

Calculate the moles of H₂O produced:

Assume complete reaction of the limiting reagent (HCl in this case).

Moles of HCl = 0.620 mol (from the information given)

Since the stoichiometric coefficient for H₂O production is 1:1 with HCl, moles of H₂O produced = 0.620 mol

Calculate ΔH per mole of H₂O produced:

ΔH = heat absorbed / moles of H₂O produced

ΔH = 1325.02 J / 0.620 mol

= 2137.13 J/mol

Therefore, the ΔH for the reaction per mole of H₂O produced is 2137.13 J/mol.