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rusak2 [61]
3 years ago
13

Give three examples, from the lab, where potential energy was converted to kinetic energy.

Chemistry
1 answer:
GREYUIT [131]3 years ago
4 0

Give 3 Examples of where potential energy was converted to knlinetic energy:

Curtain

A ball before moving

An apple from the tree then falling down

When the Curtains are still, we call the that potential energy. If you move the curtains around, that is kinetic energy

The ball is still, that is potential energy. Then the ball is moving, the is kinetic energy

There is a apple ganging from a tree, that is potential energy. That apple is fall, this is kinetic energy

Hope this helps

Don't type or write in the answer, I'm not sure what from the lab means. These are a few potential into kinetic energy I could have think of!

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Scientists ask questions, which is the basis for their investigations.
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What volume of oxygen in liters at STP wpuld be required for the combustion of 17.0 grams PH3?
Lynna [10]

First, we need to state the chemical equation for the combustion of PH3

4PH3\text{ + 8O2 }\to\text{ P4O10 }+6H2O

And the mass of PH3 is 17.0 grams and we need to know the moles.

In the periodic table, the atomic mass of the P (phosphorus) is 31 and the atomic mass of the H (hydrogen) is 1.

So, you sum the mass of P to the mass of H multiplied by 3 and you obtain this:

\text{mole}cu\text{lar weight of PH3=31}\cdot1+1\cdot3=34\text{ g PH3/mol}

With this data, we can search the moles of PH3:

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1 year ago
Does The nucleus of an atom contain all of the protons in the atom
Rina8888 [55]

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6 0
3 years ago
Use the periodic table to calculate the molar mass of each of the following compounds. Give your answer to the correct number of
Anna [14]
Fe: 2 x 55.845 = 111.69
O: 3 x 15.9994= 47.9982

111.69 + 47.9982 = 159.69 g/mol
7 0
4 years ago
How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at -154.0°C to a liquid at -42.0°C? The
WARRIOR [948]

Answer:

The answer to the question above is

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C = 29.36 kJ

Explanation:

The given variables are

ΔHfus = 7.27 kJ/mol

Cliq = 2.16 J/g°C

Cgas = 1.29 J/g°C

Csol = 1.65 J/g°C

Tmelting = -95.0°C.

Initial temperature = -154.0°C

Final temperature = -42.0°C?

Mass of acetone = 87.1 g

Molar mass of acetone = 58.08 g/mol

Solution

Heat required to raise the temperature of solid acetone from -154 °C to -95 °C or 59 °C is given by

H = mCsolT = 87.1 g* 1.65 J/g°C* 59 °C = 8479.185 J

Heat required to melt the acetone at -95 °C = ΔHfus*number of moles =

But number of moles = mass÷(molar mass) = 87.1÷58.08 = 1.5

Heat required to melt the acetone at -95 °C =1.5 moles*7.27 kJ/mol = 10.905 kJ

The heat required to raise the temperature to -42 degrees is

H = m*Cliq*T = 87.1 g* 2.16 J/g°C * 53 °C = 9971.21 J

Total heat = 9971.21 J + 10.905 kJ + 8479.185 J = 29355.393 J = 29.36 kJ

The energy required to heat 87.1 g acetone from a solid at -154.0°C to a liquid at -42.0°C is 29.36 kJ

4 0
4 years ago
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