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Klio2033 [76]
3 years ago
11

What can you infer about the volume of a gas as absolute zero is approached?

Chemistry
1 answer:
schepotkina [342]3 years ago
4 0

Answer:

The volume of a gas approaches zero as the temperature approaches absolute zero.

Step-by-step explanation:

You may have done a <em>Charles' Law experiment</em> in the lab, in which you measured the volumes of a gas at various temperatures.

You plotted them on a graph, and perhaps you were asked to extrapolate the graph to lower temperatures.

Your graph probably looked something like the one below.

There is clearly an x-intercept at some low temperature.

Inference: The volume of a gas approaches zero as the temperature approaches absolute zero.

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You have two buffered solutions. Buffered solution 1 consists of 5.0 M HOAc and 5.0 M NaOAc; buffered solution 2 is made of 0.05
andre [41]

Answer:

C

Explanation:

The Henderson-Hasselbalch equation relates pH to the concentrations of an weak acid-base conjugate pair as follows:

pH = pKa + log([A⁻]/[HA])

For solution 1, the pH may be expressed as follows:

pH = pKa + log(5.0M/5.0M) = pKa

For solution 2,  pH may be expressed as follows:

pH = pKa + log(0.050M/0.050M) = pKa

Thus, the pH values are equal to the pKa in both cases and are the same.

7 0
3 years ago
A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba 2 . When the concentration of F - exceeds __________ M,
Stella [2.4K]

Answer:

When [F⁻] exceeds 0.0109M concentration, BaF₂ will precipitate

Explanation:

Ksp of BaF₂ is:

BaF₂(s) ⇄ Ba²⁺(aq) + 2F⁻(aq)

Ksp = 1.7x10⁻⁶ = [Ba²⁺] [F⁻]²

The solution will produce BaF₂(s) -precipitate- just when [Ba²⁺] [F⁻]² > 1.7x10⁻⁶.

As the concentration of [Ba²⁺] is 0.0144M, the product [Ba²⁺] [F⁻]² will be equal to  ksp just when:

1.7x10⁻⁶ = [Ba²⁺] [F⁻]²

1.7x10⁻⁶ = [0.0144M] [F⁻]²

1.18x10⁻⁴ = [F⁻]²

0.0109M = [F⁻]

That means, when [F⁻] exceeds 0.0109M concentration, BaF₂ will precipitate

5 0
3 years ago
B) All atoms contain<br>charged electrons.<br>​
andrey2020 [161]

Answer:

b) All atoms contain

charged electrons.

Explanation:

8 0
3 years ago
How many moles of O2- ions are there in 0.450 moles of aluminum oxide, Al2O3?
Mashutka [201]

Answer:

                     1.35 moles of O²⁻

                     21.6 grams of O²⁻

Explanation:

We know that the charge on Aluminium ion is +3 (i.e. Al³⁺) while, the charge on Oxide ion is -2 (i.e. O²⁻). Therefore, the overall neutral Al₂O₃ compound has 2 Al³⁺ ions and 3 O²⁻ ions. Since, we can say that,

                 1 mole of Al₂O3 contains  =  3 moles of O²⁻ ions

So,

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Solving for X,

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As the mass of an atom is mainly due to the presence of protons and neutrons hence, the addition of two electrons (-ve 2 shows two gained electron) to Oxygen will make a negligible change to the atomic masss of Oxygen because electron is said to be almost 1800 times lighter than proton. Hence, the ionic mass of O²⁻ will be 16 g/mol and the mass of given moles is calculated as,

                     Mass  =  Moles × Ionic Mass

                     Mass  =  1.35 mol × 16 g/mol

                    Mass  =  21.6 g

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