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?

-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 =

Heat absorbed by the bomb claorimeter = Q

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.

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the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3