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3 years ago

Which scientist made the most important discovery concerning indemnifying the sun as a star

Chemistry

2 answers:

Iteru [2.4K]3 years ago

8 0

Isaac Newton was the one who made that important discovery

Studentka2010 [4]3 years ago

6 0

Answer: Isaac Newton

Isaac Newton, an English scientist, lived from 1642 to 1727. In 1665 he realized that it was gravity that held the solar system together.

Explanation:

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Rubidium has two naturally occurring isotopes, rubidium -85 ( atomic mass = 84.9118 amu; abundance = 72.15%) and rubidium -87 (a

son4ous [18]

Answer:

The answer to your question is: 85.458 amu

Explanation:

data

Rubidium-85 A = 84.9118 amu abundance = 72.15%

Rubidium - 87 A = 86.9092 amu abundance = 27.85%

Atomic weight = ?

Atomic weight = 84.9118(0.7215) + 86.9092(0.2785)

Atomic weight = 61.2538 + 24.2042

Atomic weight = 85.458 amu

6 0

4 years ago

Explain why some people use the term decimal system as a synonym for the metric system?

Luda [366]

Answer:

The term Decimal is coined from the word Decimus. Decimus is a Latin word which means ‘tenth’.

The Decimal system is a system of numbering that is based on multiples of tens. It is flexible and easy to convert from one metric to another.

The preference of the term over the Metric System is because the word Metric is related more to the measurement of lengths if we looked at the origin of the word which is French.

Cheers!

3 0

3 years ago

can someone explain in detail how molar mass, Avogadro's number, and volume are all connected through moles? Im so confused :(

sashaice [31]

Answer:

See Explanation

Explanation:

By definition, 1 mole is the mass of substance (or, formula mass in grams) containing 1 Avogadro's Number (N₀ = 6.02 x 10²³) of particles. That is ...

1 mole of hydrogen atoms (H) = 1.00794 grams

1 mole of molecular hydrogen (H₂) = 2.01588 grams

1 mole of any substance = 1 formula weight in grams

1 mole = 1 Avogadro's Number (N₀) = 1 formula weight in grams

In the concept of 'gas laws' 1 mole of any (all) gas at STP conditions ( => 0°C & 1 atmosphere pressure) occupies 22.4 Liters & is known as the 'molar volume' of a gas at STP. If the temperature &/or pressure change the volume will not be 22.4 Liters.

For reactions whose coefficients are balanced to the lowest whole number values (i.e., no fractional coefficients) the equation is known as the 'standard reaction' and conditions are assumed to be STP and the coefficients of gas phase components indicate molar volumes. Example ...

Given N₂(g) + 3H₂(g) => 2NH₃(g) is assumed to be at 0°C; 1 Atm pressure.

Molecular Nitrogen = 1 molar volume = 22.4 Liters of N₂(g)

Molecular Hydrogen = 3 molar volumes = 3 x 22.4 Liters of H₂(g) = 67.2 Liters of H₂(g)

Molecular Ammonia = 2 molar volumes = 2 x 22.4 Liters of NH₃(g) = 44.8 Liters of NH₃

8 0

3 years ago

An empty water bottle is full of air at 15°C and standard pressure. The volume of the bottle is 0.500 liter. How many moles of a

lord [1]

Answer: 0.02 moles

Explanation: Using ideal gas equation:

$PV=nRT$