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3 years ago

How many moles of S are in 35.4 g of (C3H5)2S?

1 answer:

6 0

<span>0.310 moles First, look up the atomic weights of the elements involved. Atomic weight carbon = 12.0107 Atomic weight hydrogen = 1.00794 Atomic weight sulfur = 32.065 Molar mass (C3H5)2S = 6 * 12.0107 + 10 * 1.00794 + 32.065 = 114.2086 g/mol Moles (C3H5)2S = 35.4 g / 114.2086 g/mol = 0.309959145 mol Since there's just one sulfur atom per (C3H5)2S molecule, the number of moles of sulfur will match the number of moles of (C3H5)2S which is 0.310 when rounded to 3 significant digits.</span>

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Alinara [238K]

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3 years ago

Read 2 more answers

Iron reacts slowly with oxygen and water to form a compound commonly called rust (Fe₂O₃?4H₂O). For 45.2 kg of rust, calculate

Mashcka [7]

Rust (Fe2O3. 4H2O) is formed when iron interacts slowly with oxygen and water. Mass of Fe in grams is 2.18 x 10⁴ g.

<h3>What is the explanation?</h3>

There are 2 moles of Fe atoms in 1 mole of Fe2O3-4H2O. The number of moles of Fe atoms in 45.2 kg rust is shown below.

Moles of Fe = 195.01 mol Fe₂O₃.4H₂O ( $\frac{2 mol Fe }{1 mol Fe₂O₃.4H₂O}$ )

Moles of Fe = 390.02 mol Fe

Multiply the calculated number of moles of iron, Fe, by its molar mass which is 55.85 $\frac{g}{mol}$

Mass of Fe = 390.02 mol Fe ( $\frac{55.85 g Fe}{mol Fe}$ )

Mass of Fe = 2.18 x 10⁴ g Fe

Avogadro's number (6.022 x 1023) of molecules (or formula units) make up one mole of a substance (ionic compound). The mass of 1 mole of a chemical is indicated by its molar mass. It provides you with the amount of grams per mole of a substance, to put it another way.

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brainly.com/question/26416088

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1 year ago

What do you already know about fossils? Describe as much as you can in the space below.

Wewaii [24]

Answer:

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2 years ago

Explain Any differences in the pulse rate at rest and after rest ( in your own words)

Brrunno [24]

Explanation:

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2 years ago

A reaction is followed and found to have a rate constant of 3.36 × 104 m-1s-1 at 344 k and a rate constant of 7.69 m-1s-1 at 219

g100num [7]

The relation between rate constants at different temperatures, temperature and activation energy is known as Arrhenius equation

<u>Arrhenius equation</u>

$K=Ae^-{\frac{Ea}{RT} }$

For two temperatures

$Ea=R(\frac{ln\frac{k1}{k1} }{(\frac{1}{T1})-(\frac{1}{T2})})$

Where

Ea = ? = activation energy

k1 = 3.36 × 10⁴

T1=344 k

k2=7.69

T2=219K

R= gas constant = 8.314 J /molK

Putting values

$Ea= (8.314)(\frac{ln(\frac{7.69}{33600})}{(\frac{1}{344})(\frac{1}{219})}$

Ea = (-69.69)/(-0.00166) = 41981.93 J/mol

Activation energy is 42.0 kJ /mol

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2 years ago