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2 years ago

Give the following compound's base name.

Chemistry

1 answer:

Murljashka [212]2 years ago

6 0

Answer:

2-Butyne

Explanation:

The given compound name is 2-Butyne.

According to the IUPAC rule, the compound is consist of 4 carbon atoms with triple bond at second carbon atom, so its name will be 2-Butyne or but-2-yne. 2-Butyne is an alkyne which is produced artificially at standard temperature and pressure.

Hence, the correct answer is "2-Butyne".

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With the atomic number 1 and an atomic mass of 1.0079, hydrogen has _________.

xz_007 [3.2K]

Answer: A-2 energy levels

Explanation:

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2 years ago

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He generic metal a forms an insoluble salt ab(s) and a complex ac5(aq). the equilibrium concentrations in a solution of ac5 were

elena55 [62]

Balanced chemical reaction: A + 5C ⇄ AC₅.
[A] = 0.100 M; equilibrium concentration.
[C] = 0.0380 M.
[AC₅] = 0.100 M.
Kf = [AC₅] / ([A] · [C]⁵).
Kf = 0.100 M ÷ (0.100 M · (0.0380 M)⁵.
Kf = 12620658.54 = 1,26·10⁷.
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2 years ago

What is hydrocabron

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Answer:

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2 years ago

A mouse is placed in a sealed chamber with air at 769.0 torr. This chamber is equipped with enough solid KOH to absorb any CO2 a

svlad2 [7]

Answer: The amount of oxygen gas consumed by mouse is 0.202 grams.

Explanation:

We are given:

Initial pressure of air = 769.0 torr

Final pressure of air = 717.1 torr

Pressure of oxygen = Pressure decreased = Initial pressure - Final pressure = (769.0 - 717.1) torr = 51.9 torr

To calculate the amount of oxygen gas consumed, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 51.9 torr

V = Volume of the gas = 2.20 L

T = Temperature of the gas = 292 K

R = Gas constant = $62.364\text{ L. Torr }mol^{-1}K^{-1}$

n = number of moles of oxygen gas = ?

Putting values in above equation, we get:

$51.9torr\times 2.20L=n\times 62.364\text{ L. Torr }mol^{-1}K^{-1}\times 292K\\\\n=\frac{51.9\times 2.20}{62.364\times 292}=0.0063mol$

To calculate the mass from given number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Moles of oxygen gas = 0.0063 moles

Molar mass of oxygen gas = 32 g/mol

Putting values in above equation, we get:

$0.0063mol=\frac{\text{Mass of oxygen gas}}{32g/mol}\\\\\text{Mass of oxygen gas}=(0.0063mol\times 32g/mol)=0.202g$

Hence, the amount of oxygen gas consumed by mouse is 0.202 grams.

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2 years ago

How could you use a model to show the cause-and-effect relationship between Earth's rotation and the apparent motion of the star

Masteriza [31]

Question:

How could you use a model to show the cause-and-effect relationship between Earth's rotation and the apparent motion of the stars across the night sky?

Answer:

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