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sergiy2304 [10]
2 years ago
5

Phosphorus pentachloride decomposes according to the chemical equation

Chemistry
1 answer:
Elena L [17]2 years ago
3 0

Answer:

[PCl₅]  → 4.47×10⁻³ M

[PCl₃]  → 0.0897M

Explanation:

We state the equilibrium: PCl₅ (g) ⇄  PCl₃(g) + Cl₂(g)

Initially we have 0.4192 moles of  PCl₅ so during the reaction, x moles of it have been reacted. In conclussion after the equilibrium we may have x moles of PCl₃ and Cl₂. In order to find the final concentration, we use the Kc, but we need molar concentrations. That's why we divide all the values with the 4.5L, volume for the vessel. The expression for Kc is:

Kc = [PCl₃] . [Cl₂] / [PCl₅]

1.80 = (x/ 4.45) . (x/ 4.45) / ((0.4192-x) /4.45)

1.80 = (x² / 4.45²) / ((0.4192-x) /4.45)

1.80 = x² / 4.45 / (0.4192-x)

1.80 (0.4192-x) = x² / 4.45

1.80 (0.4192-x) . 4.45 - x² = 0

3.36 - 8.01x - x² = 0 → Quadractic

a = -1  b = -8.01  c = 3.36

(-b + √(b² - 4ac)) / (2a)

(-(-8.01) + √((-8.01)² - 4(-1)3.36)) / (2(-1) = 0.3995

[PCl₅] = (0.4192 - 0.3995) / 4.45L → 4.47×10⁻³ M

[PCl₃] = 0.3995 /4.45L → 0.0897M

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Answer:

pH = 10.75

Explanation:

To solve this problem, we must find the molarity of [OH⁻]. With the molarity we can find the pOH = -log[OH⁻]

Using the equation:

pH = 14 - pOH

We can find the pH of the solution.

The molarity of Ca(OH)₂ is 2.8x10⁻⁴M, as there are 2 moles of OH⁻ in 1 mole of Ca(OH)₂, the molarity of [OH⁻] is 2*2.8x10⁻⁴M = 5.6x10⁻⁴M

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<h3>pH = 10.75</h3>
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Explanation:

To calculate the wavelength of light, we use the equation:

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Putting in the values:

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Thus the wavelength of the x-ray wave is 10^{-10}m

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