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tankabanditka [31]
3 years ago
10

Solve if an element has a charge of 2+, how many more protons does it have than electrons? protons

Chemistry
1 answer:
Effectus [21]3 years ago
8 0
To determine how many protons are present, simply know or use the following equation

X = number of protons
Y = number of electrons
Z = formal charge of the element

X - Y = Z = 0 for a neutral atom

X - Y = 2

Then to solve for x

X = Y + 2.

This means that we would need an additional 2 more protons than electrons.
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In general, in what type of solvent (non-polar, moderately polar, or highly polar) are polar solutes most soluble? Explain why.
tia_tia [17]

Answer:

  • In general, polar solutes are most soluble in highly polar solvents.

Explanation:

The general rule is "like dissolves like" which means that <em>polar solvents </em>dissolve polar (or ionic) <em>solutes</em> and <em>non-polar solvents</em> dissolve non-polar solutes.

In order for a solvent dissolve a solute, the strength of the interacttion (force) between the solute and the solvent units (atoms, molecules, or ions) must be stronger than the strength of the forces that keep together he particles of the pure substances (known as intermolecular forces).

Since the nature of the interactions between the units are electrostatic, the more polar is the solvent the better it will be able to attract and surround the solute particles, keeping them separated and in solution. That mechanism explains why polar solutes will be most soluble in highly polar solvents.

5 0
2 years ago
Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 16°
Pavel [41]

Answer:

PNO₂ = 0.49 atm

PN₂O₄ = 0.45 atm

Explanation:

Let's begin with the equation of ideal gas, and derivate from it an equation that  involves the density (ρ = m/V).

PV = nRT

n = m/M (m is the mass, and M the molar mass)

PV = \frac{m}{M}RT

PxM = \frac{m}{V}RT

PxM = ρRT

ρ = PxM/RT

With the density of the gas mixture, we can calculate the average of molar mass (Mavg), with the constant of the gases R = 0.082 atm.L/mol.K, and T = 16 + 273 = 289 K

2.7 = \frac{0.94xMavg}{0.082x289}

0.94Mavg = 63.9846

Mavg = 68.0687 g/mol

The molar mass of N is 14 g/mol and of O is 16 g/mol, than M_{NO2} = 46 g/mol and M_{N2O4} = 96 g/mol. Calling y the molar fraction:

Mavg = M_{NO2}y_{NO2} + M_{N2O4}y_{N2O4}

And,

y_{NO2} + y_{N2O4} = 1

y_{N2O4} = 1 - y_{NO2}

So,

68.0687 = 46y_{NO2} + 92x(1 - y_{NO2})

68.0687 - 92 = 46y_{NO2} - 92y_{NO2}

46y_{NO2} = 23.9313

y_{NO2} = 0.52

y_{N2O4} = 0.48

The partial pressure is the molar fraction multiplied by the total pressure so:

PNO₂ = 0.52x0.94 = 0.49 atm

PN₂O₄ = 0.48x0.94 = 0.45 atm

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The answer is.... : 5.4 atm
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