How many grams are in 1.30 x 10^24 formula units of Ca(NO3)2?
A. 151 g
B. 354 g
C. 294 g
D. 416 g
Answers
Answer:
354 gram
Explanation:
No of formula units = no of moles × Avogadro's number
Number of moles = no of formula units/ Avogadro's number
No of moles = 1.30×10^24/60.02×10^23
No of moles = 2.159 moles
Mo of moles = mass in gram/ molar mass
Mass in gram = no of moles× molar mass
Mass in gram =2.159×164
Mass in gram = 354.15 gram
The grams that are present in [tex]1.30 * 10^{24}[/tex] formula units of [tex]Ca(NO_3)_2[/tex] is 354 gram that can be calculated using number of moles.
(B) 354 g
One mole:A mole is defined as [tex]6.02214076 * 10^{23}[/tex] of some chemical unit, be it atoms, molecules, ions, or others.
No. of formula units = no of moles × Avogadro's number
Number of moles = no of formula units/ Avogadro's number
No. of moles = [tex]1.30*10^{24}/6.022*10^{23}[/tex]
No. of moles = 2.159 moles
The Number of moles is defined as the given mass over molar mass.
No. of moles = Mass / Molar mass
Mass = no. of moles× molar mass
Mass =2.159×164
Mass = 354.15 gram
Thus, option B is correct.
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Answer:
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Answer:
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I did not understand the question but hope this help!
The pH of a solution is 8.7 and pOH is 5.3
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Answer:
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Explanation:
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