The combustion of 1.5011.501 g of fructose, c6h12o6(s)c6h12o6(s) , in a bomb calorimeter with a heat capacity of 5.205.20 kj/°c results in an increase in the temperature of the calorimeter and its contents from 22.9322.93 °c to 27.4327.43 °c. what is the internal energy change, δδu , for the combustion of 1.5011.501 g of fructose?

Answer : The internal energy change is -2805.8 kJ/mol

Explanation :

First we have to calculate the heat gained by the calorimeter.

where,

q = heat gained = ?

c = specific heat =

= final temperature =

= initial temperature =

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

Now we have to calculate the enthalpy change during the reaction.

where,

= enthalpy change = ?

q = heat gained = 23.4 kJ

n = number of moles fructose =

Therefore, the enthalpy change during the reaction is -2805.8 kJ/mole

Now we have to calculate the internal energy change for the combustion of 1.501 g of fructose.

Formula used :

or,

where,

= change in enthalpy =

= change in internal energy = ?

= change in moles = 0   (from the reaction)

R = gas constant = 8.314 J/mol.K

T = temperature =

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

Therefore, the internal energy change is -2805.8 kJ/mol

The combustion of 1.501 g of fructose, C₆H₁₂O₆(s), in a bomb calorimeter with a heat capacity of 5.20 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.93 °C to 27.43 °C. What is the internal energy change, ΔU, for the combustion of 1.501 of fructose?

The combustion of 1.501 g of fructose, C₆H₁₂O₆(s), in a bomb calorimeter with a heat capacity of 5.20 kJ/°C, resulting in an increase in the temperature of the calorimeter and its contents from 22.93 °C to 27.43 °C, represents a change in the internal change for the combustion of -2.81 × 10³ kJ/mol.

A bomb calorimeter is a type of constant-volume calorimeter used in measuring the heat of combustion of a particular reaction and in determining the internal energy change (ΔU) of the combustion process.

First, we will calculate the heat absorbed by the bomb calorimeter (Qcal) using the following expression.

where,

According to the law of conservation of energy, the sum of the heat absorbed by the bomb calorimeter and the heat released by the combustion (Qcomb) is zero.

1.501 g of fructose with a molar mass of 180.16 g/mol reacted. The corresponding number of moles are:

Finally, we can calculate the change in the internal energy for the combustion reaction of fructose using the following expression.

The combustion of 1.501 g of fructose, C₆H₁₂O₆(s), in a bomb calorimeter with a heat capacity of 5.20 kJ/°C, resulting in an increase in the temperature of the calorimeter and its contents from 22.93 °C to 27.43 °C, represents a change in the internal change for the combustion of -2.81 × 10³ kJ/mol.

You can learn more about calorimetry here:

2b2t

explanation:

2b2t

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.