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4 years ago

How many moles of oxygen will occupy a volume of 2.50 at 1.20 atm and 25.0 c?

Chemistry

1 answer:

pav-90 [236]4 years ago

7 0

Answer:

The number of mol of oxygen is 0, 123

Explanation:

We use the formula PV=nRT. We convert the temperature in Celsius into Kelvin. 0°C=273 K---> 25°C=273+25= 298K

PV=nRT---> n=(PV)/(RT)

n= (1,20 atm x2,50 L)/(0,082 l atm/ K mol x 298K)

n=0,122769684 mol

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Using VSEPR theory which of the following would be the correct shape for nitrogen trifluoride?

RUDIKE [14]

Answer:

trigonal pyramidal

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In NF3, the nitrogen atom is sp3 hybridized. Now we must remember that according to the VSEPR theory, the number of electron pairs in the valence shell of the central atom in a molecule determines its shape.

Here, the nitrogen atom is the central atom and its outermost shell is surrounded by four electron pairs - one lone pair and three bond pairs. This means that it has a tetrahedral electron pair geometry.

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Covalent Bonds How many covalent bonds can Nitrogen atoms make ?

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3 years ago

Initial Concentration mol/L[A] Initial Concentration mol/L[B] Initial Rate mol/Ls 0.20 0.10 20 0.20 0.20 40 0.40 0.20 160 Given

zimovet [89]

The generalized rate expression may be written as:
r = k[A]ᵃ[B]ᵇ

We may determine the order with respect to B by observing the change in rate when the concentration of B is changed. This can be done by comparing the first two runs of the experiment, where the concentration of A is constant but the concentration of B is doubled. Upon doubling the concentration of B, we see that the rate also doubles. Therefore, the order with respect to concentration of B is 1.
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Effective nuclear charge, Zeff, is defined as:

Alborosie

Answer:

The effective nuclear charge for a valence electron in oxygen atom: $Z_{eff} = 4.55$

Explanation:

Effective nuclear charge $[Z_{eff}]$ is the net nuclear charge experienced by the electron in a given atom. It is always less than the actual charge of the nucleus [Z], due to shielding by electrons in the inner shells.

It is equal to the difference between the actual nuclear charge or the atomic number (Z) and the shielding constant (s).

$\Rightarrow Z_{eff} = Z - s$

For an oxygen atom-

Electron configuration: (1s²) (2s² 2p⁴)

The atomic number (actual nuclear charge): Z = 8

The shielding constant (s) for a valence electron can be calculated by using the Slater's rules:

⇒ s = 5 × 0.35 + 2 × 0.85 = 1.75 + 1.7 = 3.45

Therefore, the effective nuclear charge for a valence electron in oxygen atom is:

$Z_{eff} = Z - s = 8 - 3.45 = 4.55$

Therefore, the effective nuclear charge for a valence electron in oxygen atom: $Z_{eff} = 4.55$

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