Hello, 3Coli Here!
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I would recheck, redo, and revise my answers, if necessary. Also, I can look at the lesson again, if I forgot something. So that's what I would do.
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Sorry, but where are the ‘items’?
Answer:
14.77 mol.
Explanation:
- It is known that every 1.0 mole of compound or element contains Avogadro's number (6.022 x 10²³) of molecules or atoms.
<u><em>Using cross multiplication:</em></u>
1.0 mole of He contains → 6.022 x 10²³ atoms.
??? mole of He contains → 8.84 x 10²⁴ atoms.
<em>∴ The no. of moles of He contains (8.84 x 10²⁴ atoms) </em>= (1.0 mol)(8.84 x 10²⁴ atoms)/(6.022 x 10²³ atoms) =<em> 14.77 mol.</em>
Answer:
V = 38.48 L
Explanation:
Given that,
No. of moles = 1.5 mol
Pressure, P = 700 torr
Temperature, T = 15°C = 288 K
We need to find the volume of the gas. The ideal gas equation is given by :
, R = L.Torr.K⁻¹.mol⁻¹
So, the required volume is equal to 38.48 L.
Answer:
The molar mass of
is 96.8 g/mol
Explanation:
The given molecular formula - 
Individual molar masses of each element in the compound is as follows.
Molar mass of nitrogen - 14.01 g/mol
Molar mass of of hydrogen = 1.008g/mol
Molar mass of carbon = 12.01 g/mol
Molar mass of oxygen =16.00 g/mol
Molar mass of
is
![2\times[1(14.01)+4(1.008)]+1(12.01)+3(16.00)= 96.8g/mol](https://tex.z-dn.net/?f=2%5Ctimes%5B1%2814.01%29%2B4%281.008%29%5D%2B1%2812.01%29%2B3%2816.00%29%3D%2096.8g%2Fmol)
Therefore,The molar mass of
is 96.8 g/mol