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2 years ago

If there were only 4 protons, but the number of electrons remained at 6, what would the charge of this atom be? please help!!

Chemistry

1 answer:

lina2011 [118]2 years ago

5 0

Answer:

Negatively charged

Explanation:

It could be an ion too. To balance the electron shell it could lose 1 or 2 electrons. If it is not an ion it won't lose atoms to balance the shells.

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References Use the References to access important values if needed for this question A student ran the following reaction in the

ANTONII [103]

Answer:

19.27

Explanation:

Some values are corrected from correct source.Thus,

Moles of SO₂ = 8.19x10⁻² moles

Moles of O₂ = 8.10x10⁻² moles

Volume = 1 L

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

Concentration of SO₂ = 8.19x10² M

Concentration of O₂ = 8.10x10 M

Considering the ICE table for the equilibrium as:

2SO₂ (g) + O₂ (g) ⇔ 2SO₃ (g)

t = o 8.19x10⁻² 8.19x10⁻²

t = eq -2x -x 2x

--------------------------------------------- --------------------------

neq: 8.19x10⁻² -2x 8.19x10⁻² -x 2x

Given:

Equilibrium concentration of O₂ = 5.98x10⁻² M = 8.19x10⁻² -x

Thus, x = 0.0212 M

[SO₂] = 8.19x10⁻² - 2*0.0212 = 0.0395 M

[SO₃] = 2*0.0212 = 0.0424 M

The expression for the equilibrium constant is:

$K_c=\frac {[SO_3]^2}{[SO_2]^2[O_2]}$

$K_c=\frac{{0.0424}^2}{{0.0395}^2\times 0.0598}$

K = 19.27

4 0

3 years ago

What is the [H+] concentration of a solution with a pH of 3.78

lianna [129]

Answer:

[H+] = 1.66 x $10^{-4}$

Explanation:

To find the [H+] concentration of a solution, we can use the formula:

$[H+] = 10^{-pH}$

Let's plug in the pH.

$[H+] = 10^{-3.78}$

Evaluate the exponent.

[H+] = 1.66 x $10^{-4}$

Hope this helps!

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sladkih [1.3K]

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2 years ago

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Leya [2.2K]

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Explanation:

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