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2 years ago

What mass (in mg) does 2.63 moles of nickel have?

1 answer:

6 0

Atomic mass Nickel ( Ni) = 58.69 a.m.u

1 mole ------------- 58.69 g
2.63 moles -------- ??

2.63 x 58.69 / 1 => 154.3547 g

1 g ------------- 1000 mg
154.3547 g ---- ??

154.3547 x 1000 / 1

=> 154,354.7 mg

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Why don't noble gasses want to react with anyone?

Zepler [3.9K]

They have a full valence shell (8 electrons in the outer shell) so they are the most stable elements on the periodic table. Therefore, they do not need to react to other elements to gain or lose elections to become stable.

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2 years ago

What substance cannot be broken down by chemical change

ki77a [65]

Potassium is the simplest form of matter and therefore can not be broken down by chemical change.

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3 years ago

The arsenic in a 1.223 g sample of a pesticide was converted to H3AsO4 by suitable treatment. The acid was then neutralized, and

Vladimir79 [104]

Answer:

5.471% As₂O₃ in the sample.

Explanation:

...the reaction is: Ag+ + SCN- => AgSCN(s) Calculate the percent As2O3 in the sample. (F.W. As2O3 = 197.84 g/mol).

First, with the amount of KSCN we can find the moles of Ag in the filtrates. As we know the amount of Ag added we can know the precipitate of Ag and the moles of AsO₄ = 1/2 moles of As₂O₃ in the sample:

Moles KSCN = Moles Ag⁺ in the filtrate:

0.01127L * (0.100mol / L)= 0.001127moles Ag⁺

Total moles Ag⁺:

0.0400L * (0.0781mol/L) = 0.0031564 moles Ag⁺

Moles of Ag⁺ in the precipitate:

0.0031564 - 0.001127 = 0.0020294 moles Ag⁺

Moles AsO₄ = Moles As:

0.0020294 moles Ag⁺ * (1mol As / 3 moles Ag⁺) = 6.765x10⁻⁴ moles AsO₄

Moles As₂O₃:

6.765x10⁻⁴ moles AsO₄ * (1 mol As₂O₃ / 2 mol AsO₄) =

3.382x10⁻⁴ moles As₂O₃

Mass As₂O₃:

3.382x10⁻⁴ moles As₂O₃ * (197.84g/mol) = 0.0669g As₂O₃

Percent is:

0.0669g As₂O₃ / 1.223g sample * 100 =

<h3>5.471% As₂O₃ in the sample</h3>

7 0

3 years ago

Help, please!

professor190 [17]

Hi so from what I can see the pizza as a distant or and you just have to convert the grams of glucose into moles. Most teachers ask for this format

7 0

2 years ago

What is the pressure of a mixture of oxygen, nitrogen and carbon dioxide gases if the pressures of these gases are as follows: P

AleksandrR [38]

Answer:

his is an example of a first-year chemistry question where you must first convert two of the pressures to the units of the third and add them up, per Dalton’s law of additive pressures. There are three possible answers, one for each of the three pressure units.

1 atm = 760 torr …… torr and mm Hg are the same

1 atm = 101.3 kPa

Dalton’s law:

P(total) = P(O2) + P(N2) + P(CO2)

Explanation:

Gases will assume whatever pressure depending on the equation of state of the mixture (in this case) and the volume htey are contained in. That could be the ideal gas law and simple mixing law, If you are quoting the partial pressures which you call simply “the pressure” of each gas, and that these refer to their values in the present mixture, then yes, we would add them up. The pressures are low enough for the ideal gas law to apply provided the temperature is not extremely low as well .

8 0

2 years ago