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

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

Step-by-step explanation:

the heat capacity of the calorimeter is

`C_v = (q)/(\Delta T) \\\\=(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`