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3 years ago

Hermione granger is a diligent student. she wants to know what the empirical formula for c4h10 is. what is it

1 answer:

8 0

Empirical formula is the simplest ratio of whole numbers of components in a compound. While the molecular formula is the actual number of components making up the compound.
the formula given C₄H₁₀
ratio of C to H is 4:10
if we simplify this ratio;
4:10
2:5
Then the empirical formula of the compound is - C₂H₅

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The electrons in the outermost energy level are responsible for the atoms _____. These electrons are called the _______ electron

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3 years ago

An isotope with a mass number of 193 has 116 neutrons. What is the atomic number of this

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Answer:

Atomic number of this isotope = 77

Explanation:

Given that,

Mass number = 193

No of neutrons = 116

We need to find the atomic no of this isotope.

We know that,

Atomic mass = No of protons + No. of neutrons

Also, atomic no = no of protons

So,

Atomic mass = atomic no + No. of neutrons

⇒ Atomic no = Atomic mass - no of neutrons

Atomic no = 193 - 116

Atomic no = 77

Hence, 77 is the atomic no of the isotope.

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4 years ago

A certain substance X has a normal freezing point of −3.1°C and a molal freezing point depression constant =Kf·6.23°C·kgmol−1. C

muminat

Answer:

Freezing T° of solution = - 7.35 °C

Explanation:

This is about the freezing point depression, a colligative property which depends on solute.

The formula is: Freezing T° pure solvent - Freezing T° solution = m . Kf . i

Freezing T° of pure solvent is -3.1°C

At this case, i = 1. As an organic compound the urea does not ionize.

We determine the molality (mol/kg of solvent)

We convert mass to moles:

12.3 g . 1mol / 60.06 g = 0.205 moles

0.205 mol / 0.3 kg = 0.682 mol/kg

We replace data in the formula:

-3.1°C - Freezing T° of solution = 0.682 mol/kg . 6.23 kg°C/mol . 1

Freezing T° of solution = 0.682 mol/kg . 6.23 kg°C/mol . 1 + 3.1°C

Freezing T° of solution = - 7.35 °C

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4 years ago

Which one is denser? question 2 options: the earth (a solid object) the sun, which is about 300,000 times more massive than the

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4 years ago

Aluminum reacts with oxygen to form aluminum oxide. Select the correct unbalanced skeleton equation for this reaction. A. Al(s)

Natasha2012 [34]

Answer:

D. Al(s) + O₂(g) → Al₂O₃(s)

Explanation:

Aluminum is a solid metal, so it is written as Al(s).

Oxygen is a diatomic gas, so we write this compound as O₂(g).

Aluminum oxide has the formula Al₂O₃ because in oxides the oxidation number of oxygen atom is -2 and for aluminum, the oxidation number is 3. Thus, we write this compound as Al₂O₃(s).

Now, we have to found the chemical equation in which the reactants (left side) are Al(s) and O₂(g) while the product (right side) is Al₂O₃(s). From the options, we can see that the correct is (D):

Al(s) + O₂(g) → Al₂O₃(s)

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3 years ago