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

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

Explanation :

Formula used :

$q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})$

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.

$q=m\times c\times (T_{final}-T_{initial})$

$24KJ=1.30Kg\times 3.41J/g^oC\times (T_{final}-25.5)^oC$

$T_{final}=30.9^oC$

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

Answer 2

Answer:

Final temperature is 30,9°C

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!