Answer:
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Explanation:
The current temperature and pressure at <em>STP </em>(Standard Temperature and Pressure) stated by IUPAC are:
- Temperature: 273.15 K (0 °C)
- Pressure: 10⁵ Pa ≈ 0.9869 atm
Using the <em>ideal gas </em>equation, pV = nRT, and the Avogadro constant, you can find the<em> volume occupied by 5.80 × 10²⁰ molecules.</em>
![pV=nRT\\\\ \\ V=\dfrac{nRT}{p}](https://tex.z-dn.net/?f=pV%3DnRT%5C%5C%5C%5C%20%20%5C%5C%20V%3D%5Cdfrac%7BnRT%7D%7Bp%7D)
![V=\dfrac{5.80\cdot 10^{20}molec\times \dfrac{1mol}{6.022\cdot 10^{23}molec}\times 0.08206\dfrac{atm.liter}{mol.K}\times 273.15K}{0.9869atm}](https://tex.z-dn.net/?f=V%3D%5Cdfrac%7B5.80%5Ccdot%2010%5E%7B20%7Dmolec%5Ctimes%20%5Cdfrac%7B1mol%7D%7B6.022%5Ccdot%2010%5E%7B23%7Dmolec%7D%5Ctimes%200.08206%5Cdfrac%7Batm.liter%7D%7Bmol.K%7D%5Ctimes%20273.15K%7D%7B0.9869atm%7D)
![V=2.19e^{-2}liter=0.0219liter](https://tex.z-dn.net/?f=V%3D2.19e%5E%7B-2%7Dliter%3D0.0219liter)
I believe its a covalent bond?
<span>Molarity is expressed as
the number of moles of solute per volume of the solution. We calculate as follows:
2.80 g ( 1 mol / 56.11 g ) = 0.05 mol KOH
Molarity = 0.05 mol KOH / 750 mL ( 1 L / 1000 mL )
Molarity = 0.07 M
Hope this answers the question. Have a nice day.</span>
<em>1 troy ounce is equal to 0.0685714 pound.</em>
<em>1 pound is equal to 14.5833 troy ounces.</em>
14.5833 x 1795 = 26177.0235
1 pound of gold is approximately $26177.03
<u>Hopefully that helped! :)</u>