<span>(19.55 mol Au) / ( 1 ) x (196.97 g Au) / ( 1 mol Au) =
19.55 x 196.97 =
3850.76 g Au
I hope this helps you and have a great day!! :)
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Answer:
x= 138.24 g
Explanation:
We use the avogradro's number
6.023 x 10^23 molecules -> 1 mol C2H8
26.02 x 10^23 molecules -> x
x= (26.02 x 10^23 molecules * 1 mol C2H8 )/6.023 x 10^23 molecules
x= 4.32 mol C2H8
1 mol C2H8 -> 32 g
4.32 mol C2H8 -> x
x= (4.32 mol C2H8 * 32 g)/ 1 mol C2H8
x= 138.24 g
The image with the four sketches that accompany this question was obtained in internet and is attached.
Answer:
- <u>Substance X: compound</u>
- <u>Substance Y: mixture</u>
- <u>Substance W: element</u>
- <u>Substance Z: compound</u>
Explanation:
The first picture shows substance X as a matter composed by particles of one type. Every particle consists of two white balls bonded to one red ball, sketching a compound formed by two "white atoms" and one "red atom". So, this sketch shows a sample of a compound.
The second picture shows substance Y formed by two different kind of particles. One type of particles are two white balls bonded, sketching a molecule of two equal atoms, i.e. an element in the form of a diatomic molecules of a single element (likely a gas). The other type of particles are two white balls bonded to one red ball (just as in the first picture). This sketch, then, shows the mixture of one element and one compound. Thus, this is a mixture.
The third picture shows substance W formed by one type of particles: groups of two identical white balls. So, every pair of white ball sketchs a diatomic molecule, which means that this is an element (think, for example, in H₂ or O₂).
The fourth picture shows substance Z formed by groups of particles of the same type: two red balls bonded to two white balls. So, every group of these particles represents identical compounds, making this a compound and not a mixture.
Let's look at the molar weight of the answers:
NO is 30 g/mol
NO2 is 46
N2O is 44
N2O4 is 124
<span>We have the grams of the product, so we need the moles in order to calculate the molar weight. We us PV=nRT for this, assuming standard temperature and pressure. </span>
You were given the liters (.120L)
Std pressure is 1 atmosphere
You're looking for n, the number of moles
<span>Temp is 293.15 kelvin, thats standard </span>
And r is the gas constant in liters-atm per mol kelvin
(.120 liters)(1atm)=n(293.15K)(.08206)
Solving for n is .0049883835 mol
<span>.23g divided by .0049883 mol is about 46g/mol. You're answer is B I think, NO2
I hope my answer has come to your help. Thank you for posting your question here in Brainly. We hope to answer more of your questions and inquiries soon. Have a nice day ahead!
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So what we know:
-Atomic Mass = Protons + Neutrons
-Atomic Number is the number of protons
Magnesium's atomic number is 12, so the natural occurring isotope for magnesium is Mg-12 (12 protons and 12 neutrons). Added up we have an atomic mass of 24 amu. Which means if we added one neutron in Mg-13, our atomic mass would be 25 amu.
We can use the equation:
(amu of isotope 1)x + (amu of isotop 2)(x-1) = Average atomic mass
where isotope 1 is the fractional abundance we're solving for.
Plugged in it looks like this:
24x + 25(1-x) = 24.3
Now to solve for x:
24x + 25 - 25x = 24.3
-x + 25 = 24.3
-x = -.7
x = .7
So in this case, the fractional abundance of Mg-12 would be .7, or 70%.<span />
