A bomb calorimeter has a heat capacity of 2.47 kJ/K including the water. When a 0.111 g sample of ethylene (C 2H 4) was burned in this calorimeter, the temperature increased by 2.26 K. Calculate the energy of combustion for one mole of ethylene. a. -50.3 kJ/mol b. -1.41 x 103 kJ/mol c. -0.274 kJ/mol d. -624 kJ/mol e. -5.29 kJ/mol

Answer : The correct option is, (b)

Explanation :

First we have to calculate the heat produced.

where,

q = heat produced = ?

c = specific heat capacity =

= Change in temperature = 2.26 K

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

Now we have to calculate the energy of combustion for one mole of ethylene.

where,

= energy of combustion for one mole of ethylene = ?

q = heat released = 5.5822 kJ

m = mass of = 0.111 g

Molar mass of = 28 g/mol

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

Negative sign indicate the energy is released.

Therefore, the energy of combustion for one mole of ethylene is,

yes, water is wet, just as it makes other things wet, it is wet itself, kinda like ice, when ice is in water, the ice makes water cold, and ice is cold, therefore with that example, water is wet