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 : The correct option is,

Explanation :

Formula used :

where,

= heat released = 24 KJ

= mass of bomb calorimeter = 1.30 Kg

= specific heat =

= final temperature = ?

= initial temperature =

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

Therefore, the final temperature of the calorimeter is,

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!

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm