Question

A sample of ethanol (C2H6O) has a mass of
0.2301 g. Complete combustion of this sample causes the temperature of a bomb calorimeter to increase by 1.33°C. The calorimeter has a mass of 2.000 kg and a specific heat of 2.45 J/g•°C.

What is the heat of combustion for this sample?

Answer 1

Answer:

-6.517 kJ is the heat of combustion for this sample that is 0.2301 grams of ethanol.

Explanation:

Mass of bomb calorimeter = 2.000 kg = 2.000 × 1000 g = 2000. g

1 kg = 1000 g

Specific heat of bomb  calorimeter = c = 2.45 J/g°C

Change in temperature = $\Delta T=1.33^oC$

Heat absorbed by the bomb claorimeter = Q

$Q=m\times c\times \Delta T$

$=2000 g\times 2.45 J/g^oC\times 1.33^oC=6,517 J$

Heat energy released on combustion of 0.2301 grams of ethanol = Q'= -Q

Q' = -Q = -6,517 J = -6.517 kJ

1 J = 0.001 kJ

-6.517 kJ is the heat of combustion for this sample that is 0.2301 grams of ethanol.

Answer 2

Answer:

6.52

Explanation:

Right on EDG