Find δh for the combustion of ethanol (c2h6o) to carbon dioxide and liquid water from the following data. the heat capacity of the bomb calorimeter is 34.65 kj/k and the combustion of 1.752 g of ethanol raises the temperature of the calorimeter from 294.42 k to 295.92 k .

Answer : The enthalpy of combustion of ethanol is, -1366.8 KJ/mole

Explanation :

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

First we have to calculate the heat released by calorimeter.

where,

= heat released by calorimeter = ?

c = heat capacity of bomb calorimeter =

m = mass of ethanol = 1.752 g

= initial temperature of calorimeter = 294.42 K

= final temperature of calorimeter = 295.92 K

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

Now we have to calculate the moles of ethanol.

Now we have to calculate the enthalpy of combustion of ethanol.

where,

= enthalpy of combustion = ?

q = heat released = -51.98 KJ

n = number of moles used in combustion = 0.03803 mole

The negative sign indicate the heat released during the reaction.

Therefore, the enthalpy of combustion of ethanol is, -1366.8 KJ/mole

question: ray weighs 100 kilograms, his wrestling partner, bobby, weighs 50 kilograms. if ray moves at 4 m s , how fast will bobby have to run at him to apply an equal amount of kinetic energy?

answer: 8 m/s he needs to run twice as fast to keep up so he has some work to do

explanation:   if the mass has units of kilograms and the velocity of meters per second, the kinetic energy has units of kilograms-meters squared per second squared.

question answered by

(jacemorris04)