Answer : The thermal energy produced during the complete combustion of one mole of cymene is -7193 kJ/mole
Explanation :
First we have to calculate the heat released by the combustion.
where,
q = heat released = ?
= specific heat of calorimeter = 
= change in temperature = 
Now put all the given values in the above formula, we get:
Thus, the heat released by the combustion = 70.43 kJ
Now we have to calculate the molar enthalpy combustion.
where,
= molar enthalpy combustion = ?
q = heat released = 70.43 kJ
n = number of moles cymene = 
Therefore, the thermal energy produced during the complete combustion of one mole of cymene is -7193 kJ/mole
The study of metals and the process for refining and making things from them is called metallurgy.
Metallurgy is said to be the scientific study both of the extraction and refining process of metals from their ores.
This process includes steps such as grinding of the ore also called ore pulverization.
Ore is crushed to increase its surface area for purpose of increasing the level of its reactivity.
Sometimes, the ore is heated in the presence of oxygen to turn the ore into and oxide. This process is known as roasting.
The "Imported Asset" refers to the image attached to this answer. And this is a true or false question regarding whether the structure shown is a cyclohexane ring containing two attached methyl groups.
The correct answer is
TRUE. The ring structure is composed of 6 carbons which makes it a cyclohexane, and there are two methyl groups (-CH3) attached to the ring in the 1- and 3-positions of the ring. The full name of this structure is 1,3-dimethylcyclohexane.
<u>Given:</u>
MilliMoles of N2 = 2.5 mmol = 0.0025 moles
Initial volume V1 = 42 cm3
Final volume V2 = 600 cm3
Temperature T = 300 K
<u>To determine:</u>
The change in Gibbs free energy, ΔG
<u>Explanation:</u>
The change in Gibbs free energy is related to the ration of the volumes:
ΔG = -nRTln(V2)/(V1)
= -0.0025*8.314*300*ln(600/42) = -16.582 J/mol
Ans: The Gibbs free energy for the process is 0.0166 kJ/mol
