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White raven [17]
3 years ago
7

For neon, determine the moles and mass contained in a 29.9−L volume at a pressure of 481.1 torr at a temperature of 300.0 K.

Chemistry
1 answer:
kondor19780726 [428]3 years ago
8 0

Answer:

.7689 mol

15.516 g

Explanation:

Use the Ideal Gas Law, PV = nRT.

Make sure to use the correct ideal gas constant R. You can either put R in torr, or you can change the pressure to atm. I've just used the torr ideal gas constant.

481.1 torr * 29.9 L = n 62.364 LTorr/molK * 300 K

14384.89 = 18709.2n

n = <u>.7689 mol</u>

The molar mass of neon (remember that neon gas = Ne, it's not diatomic) is 20.18 g/mol from the periodic table.

.7689 mol * 20.18 g/mol = <u>15.516 g</u>

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What element has an atomic mass 4?
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Which type of reaction is represented by this graph?
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D. Exothermic.  

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Hello there!

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2 years ago
A 100.0 mL solution containing 0.923 gof maleic acid (MW=116.072 g/mol) is titrated with 0.265 M KOH. Calculate the pH of the so
Vlad1618 [11]

Answer:

pH = 9,57

[M²⁻] = 7,948x10⁻²M

[HM⁻] = 4x10⁻⁵M

[H₂M] = 0M

Explanation:

The moles of maleic acid presents in the solution are:

0,923g×\frac{1mol}{116,072g}=7,952x10⁻³moles of H₂M

60,0mL of 0,265M KOH are:

0,0600L×\frac{0,265mol}{1L}=0,0159 moles of KOH

The reactions of maleic acid (H₂M) and then with HM⁻ are:

H₂M + KOH → HM⁻ + H₂O + K⁺ (1)

HM⁻ + KOH → M²⁻ + H₂O + K⁺ (2)

For a complete transformation of H₂M in HM⁻ there are necessaries 7,952x10⁻³moles of KOH. As the moles of KOH are 0,0159 moles, the restant moles are:

0,0159 - 7,952x10⁻³ = <em>7,948x10⁻³ moles of KOH</em>

By (2), the moles produced of M²⁻ are the same as moles of KOH, <em>7,948x10⁻³  moles, </em>and moles of HM⁻ are:

7,952x10⁻³ -<em> </em>7,948x10⁻³ <em> = 4x10⁻⁶ moles of HM⁻</em>

Using Henderson-Hasselbalch formula:

pH = pka + log₁₀ [M²⁻] /[HM⁻]

pH = 6,27 + log₁₀ <em>7,948x10⁻³ / 4x10⁻⁶</em>

pH = 9,57

The moles of M²⁻ are 7,948x10⁻³  and volume of the solution is 0,1000L,

[M²⁻] = 7,948x10⁻²M

Moles of HM⁻ are 4x10⁻⁶:

[HM⁻] = 4x10⁻⁵M

And there is not H₂M:

[H₂M] = 0M

I hope it helps!

8 0
3 years ago
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