Question

Complete combustion of a 0.600-g sample of a compound in a bomb calorimeter releases 24.0 kJ of heat. The bomb calorimeter has a mass of 1.30 kg and a specific heat of 3.41 J/(gi°C). If the initial temperature of the calorimeter is 25.5°C, what is its final temperature? Use mc026-1.jpg. 30.9°C 34.5°C 44.0°C 51.5°C

Answer 1

Final temperature is 30,9°C

Step-by-step explanation:

A bomb calorimeter is an instrument that allows the determination of the heat of combustion of a reaction. The heat q is defined as:

q = C×m×ΔT (1)

Where:

C is specif heat of calorimeter (3,41 J/g°C)

m is mass (1,3kg ≡ 1300g)

And ΔT is final temperature - initial temperature (X-25,5°C) X is final temperature

And q is heat (24,0kJ ≡ 24000J)

Replacing in (1):

24000J = 3,41J/g°C×1300g×(X-25,5°C)

5,41 = X-25,5°C

25,5°C + 5,41 = X

30,91°C = X

Final temperature is 30,9°C

I hope it helps!

Answer 2

Answer : The correct option is,
`30.9^oC`

Explanation :

Formula used :

`q=m* c* \Delta T=m* c* (T_(final)-T_(initial))`

where,

`q` = heat released = 24 KJ

`m` = mass of bomb calorimeter = 1.30 Kg

`c` = specific heat =
`3.41J/g^oC`

`T_(final)` = final temperature = ?

`T_(initial)` = initial temperature =
`25.5^oC`

Now put all the given values in the above formula, we get the final temperature of the calorimeter.

`q=m* c* (T_(final)-T_(initial))`

`24KJ=1.30Kg* 3.41J/g^oC* (T_(final)-25.5)^oC`

`T_(final)=30.9^oC`

Therefore, the final temperature of the calorimeter is,
`30.9^oC`