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Answer:
-514 kJ/mol
Explanation:
The bond enthalpy which is also known as bond energy can be defined as the amount of energy needed to split one mole of the stated bond. The change in enthalpy of a given reaction can be estimated by subtracting the sum of the bond energies of the reactants from the sum of the bond energies of the products.
For the given chemical reaction, the change in enthalpy of the reaction is:
Δ [2(409) + 4(388) + 3(496) - 4(630) - 4(463)] kJ/mol = 818 + 1552 + 1488 - 2520 - 1852 = -514 kJ/mol
Answer:
In the kinetic molecular theory, the molecules of an ideal gas are in constant random motion inside the container of the gas, and the pressure of the gas (which is the pressure exerted by the molecules in their collisions with the walls of the container) arise from this random motion of the molecules.
The main assumptions of the kinetic theory of gases are:
- The gas consists of a large number of molecules that collide between each other and the walls of the container; all these collisions are elastic
- The duration of the collisions is negligible compared to the time between the collisions
- The number of molecules is so large that statistics can be applied
- Intermolecular forces between the molecules are negligible (except during the collisions)
- The volume of the molecules is negligible compared to the volume of the container
In particular, the pressure of the gas is directly proportional to the average kinetic energy of the molecules, according to the equation:
where
p is the pressure of the gas
V is the volume of the container
K is the average kinetic energy of the molecules in the gas
We see that as the pressure is higher, the higher the kinetic energy of the particles: this means that the molecules will move faster, on average.
Therefore in this problem, the gas that exerts a pressure of 1.5 atm will have molecules moving faster than the molecules of the gas exerting a pressure of only 1.0 atm.