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3 years ago

How many atoms are in 0.75 moles of CH4?

Chemistry

1 answer:

Anastasy [175]3 years ago

6 0

Answer:

Explanation:

Thus, if we have 6.022 × 10 23 O atoms, we say we have 1 mol of O atoms. If we have 2 mol of Na atoms, we have 2 × (6.022 × 10 23) Na atoms, or 1.2044 × 10 24 Na atoms. Similarly, if we have 0.5 mol of benzene (C 6H 6) molecules, we have 0.5 × (6.022 × 10 23) C 6H 6 molecules, or 3.011 × 10 23 C 6H 6 molecules.

For example the atomic mass of methane (CH4)is 12 amu for the carbon plus 4 x 1 amu for the four hydrogens, for a total of 16 amu. Therefore the molar mass of methane is 16g. We say that one mole of methane has a mass of 16 g, and that there are 6.022 x 1023 atoms in that mass of methane.

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Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M. HCl. Calculate the PH after the following volumes of titrant have

DedPeter [7]

Answer:

pH will always be less than 7

Explanation:

This is because NH3 is a relatively weak base and the resulting Acidic salt on titration might hydrolyse to form a buffer solution

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3 years ago

How is the structure of the atom arranged?

In-s [12.5K]

Answer:

An atom is a complex arrangement of negatively charged electrons arranged in defined shells about a positively charged nucleus. This nucleus contains most of the atom's mass and is composed of protons and neutrons (except for common hydrogen which has only one proton).

Explanation:

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3 years ago

During mitosis, this structure moves individual chromosomes?

stiv31 [10]

Answer:

Anaphase

Explanation:

Two separate classes of movements occur during anaphase. During the first part of anaphase, the kinetochore microtubules shorten, and the chromosomes move toward the spindle poles. During the second part of anaphase, the spindle poles separate as the non-kinetochore microtubules move past each other.

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3 years ago

How many moles are in 17.2g k2s

Natalija [7]

Answer: 0.156 mol

Explanation:

To find the moles of 17.2 g K₂S, we need to know the molar mass to convert.

$17.2g*\frac{mol}{110.256 g} =0.156 mol$

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4 years ago

At 85°C, the vapor pressure of A is 566 torr and that of B is 250 torr. Calculate the composition of a mixture of A and B that b

Phantasy [73]

Answer:

Composition of the mixture:

$x_{A} =0.652=65.2$ %

$x_{B} =0.348=34.8$ %

Composition of the vapor mixture:

$y_{A} =0.809=80.9$ %

$y_{B} =0.191=19.1$ %

Explanation:

If the ideal solution model is assumed, and the vapor phase is modeled as an ideal gas, the vapor pressure of a binary mixture with $x_{A}$ and $x_{B}$ molar fractions can be calculated as:

$P_{vap}=x_{A}P_{A}+x_{B}P_{B}$

Where $P_{A}$ and $P_{B}$ are the vapor pressures of the pure compounds. A substance boils when its vapor pressure is equal to the pressure under it is; so it boils when $P_{vap}=P$ . When the pressure is 0.60 atm, the vapor pressure has to be the same if the mixture is boiling, so:

$0.60*760=P_{vap}=x_{A}P_{A}+x_{B}P_{B}\\456=x_{A}P_{A}+(1-x_{A})P_{B}\\456=x_{A}*(P_{A}-P_{B})+P_{B}\\\frac{456-P_{B}}{P_{A}-P_{B}}=x_{A}\\\\\frac{456-250}{566-250}=x_{A}=0.652$

With the same assumptions, the vapor mixture may obey to the equation:

$x_{A}P_{A}=y_{A}P$ , where P is the total pressure and y is the fraction in the vapor phase, so:

$y_{A} =\frac{x_{A}P_{A}}{P}=\frac{0.652*566}{456} =0.809=80.9$ %

The fractions of B can be calculated according to the fact that the sum of the molar fractions is equal to 1.

7 0

3 years ago