Problem: In a constant-pressure calorimeter, 70.0 mL of 0.320 M Ba(OH) 2 was added to 70.0 mL of 0.640 M HCl. The reaction caused the temperature of the solution to rise from 22.94°C to 27.30°C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·°C, respectively), what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

FREE Expert Solution

Determine the ΔH by calculating for the heat involved using the calorimetry equation   and stoichiometry.


For this problem, follow these steps:

1. Find mass of solution

2. Find the change in temperature

3. Find heat (Q)

4. Calculate moles of H2O produced
5. Find heat released

97% (366 ratings)
View Complete Written Solution
Problem Details

In a constant-pressure calorimeter, 70.0 mL of 0.320 M Ba(OH) 2 was added to 70.0 mL of 0.640 M HCl. The reaction caused the temperature of the solution to rise from 22.94°C to 27.30°C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·°C, respectively), what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equation concept. You can view video lessons to learn Thermochemical Equation. Or if you need more Thermochemical Equation practice, you can also practice Thermochemical Equation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Anliker's class at IUPUI.