Entropy is the randomness of a system. At the molecular level, entropy can be described in terms of the possible number of different arrangements of particle positions and energies, called microstates. The more microstates the system has, the greater its entropy.
Another way of looking at entropy is that the universe is moving toward a broader distribution of energy. The universe has a constant amount of energy as stated in the first law of thermodynamics. The universe started with low entropy (concentrated in the moment before the "big bang") and the entropy has since been constantly increasing by distributing this energy. Heat distribution from high temperature to low temperature is a another example of this phenomenon.
Rank these systems in order of decreasing entropy.
Rank from highest to lowest entropy. To rank items as equivalent, overlap them.
a) 1/2 mol of helium gas at 273K and 20L
b) 1/2 mol of helium gas at 100K and 20L
c) 1 mol of hydrogen gas at 273K and 40L
d) 1 mol of helium gas at 273K and 20L
e) 1/2 mol of liquid helium at 100K
f) 1 mol of helium gas at 273K and 40L
g) 1 mol of methane gas at 273K and 40L
Another way of looking at entropy is that the universe is moving toward a broader distribution of energy. The universe has a constant amount of energy as stated in the first law of thermodynamics. The universe started with low entropy (concentrated in the moment before the "big bang") and the entropy has since been constantly increasing by distributing this energy. Heat distribution from high temperature to low temperature is a another example of this phenomenon.
Rank these systems in order of decreasing entropy.
Rank from highest to lowest entropy. To rank items as equivalent, overlap them.
a) 1/2 mol of helium gas at 273K and 20L
b) 1/2 mol of helium gas at 100K and 20L
c) 1 mol of hydrogen gas at 273K and 40L
d) 1 mol of helium gas at 273K and 20L
e) 1/2 mol of liquid helium at 100K
f) 1 mol of helium gas at 273K and 40L
g) 1 mol of methane gas at 273K and 40L