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3 years ago

5

Please help me this is an easy science question where you put the correct lettered answer in the small chart. Please help you ge

t many points!

1 answer:

Elanso [62]3 years ago

4 0

Where is the picture? And the question?

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At 24°C, Kp = 0.080 for the equilibrium: NH4HS (s) NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and al

miss Akunina [59]

Answer:

Partial pressure of ammonia is 0,28.

Explanation:

For the reaction:

NH₄HS(s) ⇄ NH₃(g) + H₂S(g)

kp = 0,080 is defined as:

0,080 = P[NH₃] P[H₂S] <em>(1)</em>

Where P[NH₃] is partial pressure of NH₃

Asuming amount of NH₄HS is 1, equilibrium concentration for each compound is:

[NH₄HS] = 1 - x

P [NH₃] = x

P [H₂S] = x

Replacing in (1):

0,080 = X×X

0,080 = X²

X = 0,28 = P[NH₃]

I hope it helps

7 0

2 years ago

Una molécula de O2 esta hecho de

Airida [17]

Dos átomos de oxígeno

8 0

3 years ago

Which of the following interactions are generally considered to be unfavorable? Group of answer choices a)Interaction between Ly

Anarel [89]

Answer:

d) Interaction between Arg and Lys side chains at a pH of 7, assuming standard pKa values for Arg and Lys.

Explanation:

Arginine and Lysine are basic amino acids. They play same role in various membrane proteins. They both have high aqueous values which give rise to high electrostatic interaction. The interaction is mainly in the cations of the side chains. They both are heterologous secreted proteins which plays role of metabolite.

7 0

3 years ago

An acetic acid buffer solution is required to have a pH of 5.27. You have a solution that contains 0.010 mol of Acetic acid. Wha

dlinn [17]

Answer:

Molarity of sodium acetate you will need to add is 0.0324M

Explanation:

<em>Assuming volume of the buffer is 1L.</em>

<em />

The pH of a buffer can be determined using Henderson-Hasselbalch equation:

pH = pKa + log [A⁻] / [HA]

<em>Where pKa is pKa of the weak acid, [A⁻] molar concentration of conjugate base and [HA] molar concentration of weak acid</em>

<em />

Replacing for the acetic buffer (pKa = 4.76):

pH = 4.76 + log [Sodium Acetate] / [Acetic Acid]

As you have 0.010 moles of acetic acid in 1L:

[Acetic Acid] = 0.010mol / 1L = 0.010M

And you require a pH of 5.27:

5.27 = 4.76 + log [Sodium Acetate] / [0.010M]

0.51 = log [Sodium Acetate] / [0.010M]

10^0.51 = [Sodium Acetate] / [0.010M]

3.236 = [Sodium Acetate] / [0.010M]

3.236 [0.010M] = [Sodium Acetate]

0.0324M = [Sodium Acetate]

<h3>Molarity of sodium acetate you will need to add is 0.0324M</h3>

<em />

7 0

2 years ago

Why do ionic compounds have high melting points?

Vika [28.1K]

These oppositely charged compounds are strongly held by electrostatic forces of attraction as these be together for a long time the rise in temparature occurs so that the the melting points rises in them.

4 0

3 years ago