Question

Next, a chemical reaction of interest was conducted in the same constant volume calorimeter. The neutralization reaction of HCl(aq) with NaOH(aq) caused the temperature of the calorimeter to rise by 2.46 °C. What is the change in internal energy ΔU of the neutralization reaction in kJ?

Answer 1

Answer:

A constant volume calorimeter (bomb calorimeter) was calibrated by performing in it a reaction in which 5.23 kJ of heat energy was released, causing the calorimeter to rise by 7.33 °C. What is the heat capacity Cy of the calorimeter

Explanation:

the heat capacity of the calorimeter is

$C_v = \frac{q}{\Delta T} \\\\=\frac{5.23}{7.33} \\\\=0.714kJ /^\circ C$

Now that our  heat capacity of the calorimeter is 0.714kJ/°C

we can easily calculate  the change in internal energy ΔU of the neutralization reaction

$\Delta U = C_v \ dt$

or

$\Delta U = C_V \Delta T$

Δ T = 2.46 °C

$C_v = 0.714 kJ/ ^\circ C$

$\Delta U = 0.714*2.46\\\\=1.7564kJ$