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solong [7]
4 years ago
6

Uranus was the first planet to be discovered using a telescope. true or false

Chemistry
2 answers:
mixer [17]4 years ago
8 0

Answer:

True

Explanation:

Uranus was the first planet to be discovered by means of a telescope. This planet was viewed with a telescope in 1781 by William Herchel.

Uranus had already been visualized before its discovery as a planet, but it was not given the proper importance, because everyone who viewed it thought it was a star and not a planet. There have been records of uranus visualization since 1690, but telescope visualization was not made until 1781.

slava [35]4 years ago
7 0
Sir William Herschel announced its discovery on 13 March 1781, expanding the known boundaries of the Solar System for the first time in history and making Uranus the first planet discovered with a telescope.
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What word is used to refer to a group of organ systems working together?
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1

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in my opinion,The answer would be organism

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As the sun heats the surface of the ocean, two layers of water result. What separates the layers.
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4 years ago
if a gas is pumped from a smaller container to a container that is twice size, what happens to the pressure of the gas?
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8 0
3 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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