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4 years ago

why does a large lake filled with cool water have more thermal energy than a small pond filled with warmer water

1 answer:

8 0

Because the scale is much larger, and a larger pool can collect more energy than a small pool, and it is more likely that it would have more energy spread throughout it.

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The reason it takes so much heat to melt ice or evaporate water is that extra energy is required to break _______ bonds between

mart [117]

It takes so much heat to melt ice or evaporate water because extra energy is required to break the hydrogen bonds between water molecules.

<h3>Hydrogen bond</h3>

Hydrogen bonding is an electrostatic force of attraction between a hydrogen atom found between a pair of other atoms having a high affinity for electrons.

Hydrogen bonds cause water to be exceptionally attracted to each other creating cohesion.

It takes so much heat to melt ice or evaporate water because extra energy is required to break the hydrogen bonds between water molecules.

Find out more on Hydrogen bond at: brainly.com/question/12798212

4 0

2 years ago

The equation 2al(s) + 3br2(l) → 2albr3(s) is a(n) ______________ reaction.

Svetach [21]

Combination
Hope this helps :)

7 0

4 years ago

If an atom has six electrons how many protons does it have

Sergio039 [100]

6 protons it have to be neutral

7 0

3 years ago

What does the slope of a distance vs time graph tell you? yes

bonufazy [111]

Answer:

an increase of acceleration or decrease of acceleration

Explanation:

5 0

3 years ago

A sample of octane burns releasing 2290 J of heat to the surroundings, and the gases produced expands against a piston to do 560

dexar [7]

<u>Answer:</u> The internal energy change for the reaction is -2850 J

<u>Explanation:</u>

<u>Sign convention of heat:</u>

When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.

<u>Sign convention of work:</u>

Work done for expansion process is taken as negative and work done for compression is taken as positive.

According to the First law of thermodynamics,

$\Delta U=q+w$

where,

$\Delta U$ = internal energy

q = heat absorbed or released = -2290 J

w = work done = -560 J

Putting values in above equation, we get:

$\Delta U=(-2290)+(-560)\\\\\Delta U=-2850J$

Hence, the internal energy change for the reaction is -2850 J

4 0

4 years ago