<span>(NH4)2CO3 -> 96.09 g/mol
(6.995g ammonium carbonate)(1mol ammonium carbonate/ 96.09 g ammonium carbonate) = 0.072796 mol ammonium carbonate
In this calculation, the unit 'grams' cancels out as it's present in both the numerator and the denominator, leading to 'mol' being the remaining unit.
Examining the formula (NH4)2CO3, it can be interpreted as:
2 mol (NH4) + 1 mol (CO3) = 1 mol (NH4)2CO3
This means every mole of ammonium carbonate yields one mole of carbonate ions and two moles of ammonium ions.
(0.072796 mol ammonium carbonate) = (0.072796 mol carbonate ion) + (0.363981 mol ammonium ion) </span>
Answer:
The correct choice is: option A.
Justification:
To address this inquiry, we need to evaluate the total number of electrons each orbital can accommodate.
Orbital Number of electrons
s 2
p 6
d 10
f 14
Provided options:
A. 1s² 2s² 2p⁶ 3s² This configuration is valid as it aligns with the permitted number of electrons in each orbital and follows the correct sequence.
B. 1s² 2s² 2p⁶ 3s² 3d⁴ This configuration is not accurate because
3d⁴ should follow 3p.
C. 1s² 2s² 2d¹⁰ 2p³ This is incorrect since 2d¹⁰ is not a valid orbital.
D. 1s² 2s^s 2p³ 2d¹⁰ This option contains two errors; s as an exponent does not exist, and 2d¹⁰ is also an invalid description.
The molecular formula is C2H6O2
Attached is the solution:
Initially, convert the mass into moles.
Then, divide each mole by the smallest amount to identify the number of atoms in the empirical formula.
Next, calculate the empirical formula mass.
Then, determine the molecular formula by dividing the molar mass by the empirical formula mass.
Finally, multiply the empirical formula by the obtained answer to arrive at the molecular formula of the compound.
