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1 answer:
Answer: The statement, average kinetic energy of the gas particles is greater in container A because its particles move faster is correct.
Explanation:
Kinetic energy is the energy obtained due to the motion of an object or substance.
where,
T = temperature
This means that kinetic energy is directly proportional to temperature.
So, when heat is provided to container A then its molecules will start to move rapidly from one place to another which will cause more collisions between the atoms.
Hence, average kinetic energy will be more in container A.
Whereas container B is placed at room temperature which is low than that in container A. So, molecules in container B will move at almost same speed and therefore, specific collisions will be there. So, average kinetic energy in container B will be less than that in container A.
Thus, we can conclude that the statement, average kinetic energy of the gas particles is greater in container A because its particles move faster is correct.
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Answer:
The new temperature of the nitrogen gas is 516.8 K or 243.8 C.
Explanation:
Gay-Lussac's law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of collisions with the walls increases, that is, the pressure increases. That is, the pressure of the gas is directly proportional to its temperature.
Gay-Lussac's law can be expressed mathematically as follows:
Where P = pressure, T = temperature, K = Constant
You want to study two different states, an initial state and a final state. You have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment. By varying the temperature to a new value T2, then the pressure will change to P2, and the following will be fulfilled:
In this case:
- P1= 2 atm
- T1= 50 C= 323 K (being 0 C= 273 K)
- P2= 3.2 atm
- T2= ?
Replacing:
Solving:
T2= 516.8 K= 243.8 C
<u><em>The new temperature of the nitrogen gas is 516.8 K or 243.8 C.</em></u>