Enormous O unpredictability is in reference to the most exceedingly terrible conceivable development rate of the calculation. So O(N log N) implies that it will never keep running in some time more terrible than O(N log N). So in spite of the fact that Al's calculation scales superior to Bob's quadratic algo, it doesn't really mean it is better for ALL info sizes.
Maybe there is critical overhead in building up it, for example, making a lot of clusters or factors. Remember that even an O(N log N) calculation could have 1000 non settled circles that official at O(N) and still be viewed as O(N log N) the length of it is the most exceedingly awful part.
The ball will have kinetic energy because the released the potential and kinetic is taking over.
Answer:
The energy will be flowing from hot coffee to ice cube. The energy flow will stop when both temperatures of coffee and ice cube will become equal.
Explanation:
The second law of thermodynamics deals with the direction in which spontaneous processes go. Many processes run spontaneously in one direction, that is, they are irreversible under certain conditions. Although irreversibility is seen in everyday life, for example, a broken glass does not return to its original state, complete irreversibility is a statistical statement that cannot be seen during the life of the universe. More specifically, an irreversible process is a process that depends on the route. If the process can only go in one direction, the reverse path is fundamentally different and the process can't be reversible. For example, heat always involves the transfer of energy from a higher temperature to a lower temperature. A cold object that comes in contact with a hot object never cools, transfers heat to the hot object, and heats it up.
The answer is higher.
You should know that the London dispersion force is the weakest intermolercular attractive force while the hydrogen bonds form a high attractive intermolecular force, so you have to expect that in molecules forming hydrogen bonds the molecules will be more attached to each other than in similar-sized molecules that interact by London dispersion forces only, which takes you to conclude that the melting point of the molecules forming hydrogen bonds will be higher.
Answer:
Explanation:
Given: Entropy of surrounding: ΔSsurr = ?
Temperature: T= 355 K
The change in enthalpy of reaction: ΔH = -114 kJ
Pressure: P = constant
As we know, ΔH = -114 kJ ⇒ negative
Therefore, the given reaction is an exothermic reaction
Therefore, Entropy of surrounding at <em>constant pressure</em> is given by,
<u><em>In the given reaction:</em></u>
2NO(g) + O₂(g) → 2NO₂(g)
As, the number of moles of gaseous products is less than the number of moles of gaseous reactants.
As we know, <em>for a spontaneous process, that the total entropy should be positive.</em>
<u>Therefore, at the given temperature,</u>
- if then the given reaction is spontaneous
- if then the given reaction is non-spontaneous