Consider the reaction c12h22o11(s)+12o2(g)→12co2(g)+11h2o (l) in which 10.0 g of sucrose, c12h22o11, was burned in a bomb calorimeter with a heat capacity of 7.50 kj/∘c. the temperature increase inside the calorimeter was found to be 22.0 ∘c. calculate the change in internal energy, δe, for this reaction per mole of sucrose. express the change in internal energy in kilojoules per mole to three significant figures.

Answer : The internal energy change for 1 mole of sucrose is

Explanation :

First we have to calculate the heat released by calorimeter.

where,

= heat released by calorimeter = ?

c = heat capacity of bomb calorimeter =

= change in temperature of calorimeter =

Now put all the given values in the above formula, we get

Now we have to calculate the moles of sucrose.

Now we have to calculate the internal energy change.

As we know that, bomb calorimeter carried out at constant volume condition.

here,

So,

Now we have to calculate the internal energy change for 1 mole of sucrose.

Therefore, the internal energy change for 1 mole of sucrose is

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