The correct statement is that the average kinetic energy of the gas particles is greater in container A because its particles move faster.
<h3>What is the relation between temperature & kinetic energy?</h3>
Kinetic energy of any particle is directly proportional to the temperature of the sample of that particle.
From the given diagram, it is clear that:
- In beaker A, heat is supplied to the beaker due to which temperature of the beaker A increases as a result of it particles of gases will move with faster velocity because kinetic energy of the gases particle increases.
- Beaker B is present at room temperature, so particles in this beaker will have less velocity as compared to beaker A.
Hence, the average kinetic energy of the gas particles is greater in container A because its particles move faster.
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I'm pretty sure that it is C. :)
Answer:
Question: The Haber-Bosch process involves the combination of nitrogen and hydrogen at high temperatures in the presence of a catalyst to produce ammonia. It is currently the main industrial source of ammonia.
Explanation:
From the Law of Boyle for gases you know that the pressure and the volume of gases are inversely related. That, means that you can state PV = constant. And that implies that if P has a linear relation with the number of particles (which is what the straight line means), then V has the same kind of relation.<span> So, the relationship of volume and number of partilces will have a similar graph.</span>