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2 years ago

What is the pressure in a 27.0-L cylinder filled with 44.9 g of oxygen gas at a temperature of 315 KK

Chemistry

1 answer:

steposvetlana [31]2 years ago

6 0

Answer:

1.343 atm

Explanation:

We are given the following;

Pressure, p = ?

Volume v = 27 L

Mass of oxygen = 44.9 g

Temperature, T = 315 K

The formular relating all these variables is the equation;

PV = nRT

where R = gas constant = 0.08206 L atm / mole K

To obtain n, we use;

number of moles, n = Mass / molar mass = 44.9 / 32 = 1.403 moles

From the ideal gas equation;

P = nRT / V

P = 1.403 * 0.08206 * 315 / 27

P = 36.27 / 27 = 1.343 atm

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What is a substance's melting point?

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A melting point of a substance is a point at which the sample or substance start converting in liquid. For most substances, melting and freezing points are approximately equal. For example, the melting point and freezing point of mercury is 234.32 kelvins (−38.83 °C or −37.89 °F). Hope this helped!! :)

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3 years ago

CH3COOH  CH3COO– + H+

Oxana [17]

(a)

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; (b)

[

]

1.00

-4

mol/dm

; (c)

[

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0.16 mol⋅dm

-3

Explanation:

(a) pH of aspirin solution

Let's write the chemical equation as

⇌

I/mol⋅dm

-3

0.05

C/mol⋅dm

-3

E/mol⋅dm

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0.05 -

[

]

[

]

[

]

0.05 -

3.27

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Check for negligibility

0.05

3.27

-4

153

400

∴

is not less than 5 % of the initial concentration of

[

]

We cannot ignore it in comparison with 0.05, so we must solve a quadratic.

Then

0.05

−

3.27

-4

3.27

-4

(

0.05

−

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1.635

-5

−

3.27

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3.27

-4

−

1.635

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1.68

-5

[

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mol/L

1.68

-5

mol/L

-log

[

]

-log

(

1.68

-5

)

4.77

(b)

[

]

at pH 4

[

]

-pH

mol/L

1.00

-4

mol/L

in the buffer

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[

]

log

(

[

]

[

]

)

4.00

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log

(

[

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0.05

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3.49

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(

[

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0.05

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log

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[

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0.05

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0.51

[

]

0.05

0.51

3.24

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]

0.05

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2 years ago

A student is asked to determine the molarity of a strong base by titrating it with 0.250 M solution of H2SO4. The students is in

tamaranim1 [39]

Answer:

The molarity of the strong base is 0.625 M

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⇒ Using a buret with a tip filled with air rather than the H2SO4 solution

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Step 1: Data given

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The initial buret reading is 5.00 mL

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30.00 mL - 5.00 mL = 25.00 mL

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0.250 M = 0.250 mol/L

Since there are 2 H+ ions per H2SO4

0.250 mol/L * 2 = 0.500 mol/L

The number of moles H2SO4 = 0.500 mol/L * 0.025 L

Number of moles H2SO4 = 0.0125 mol

Step 4: Calculate moles of OH-

For 1 mol H2SO4, we need 1 mol of OH-

For 0.0125 mol of H2SO4, we have 0.0125 mol of OH-

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Molarity = moles / volume

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⇒ Using a buret with a tip filled with air rather than the H2SO4 solution

5 0

3 years ago