Respuesta :
Answer:
It is 4.09 g (NH4)2S
Explanation:
after getting the right amount of significant figures
The mass of ammonium sulfide (NH4)2S in 3.00 L of a 0.020 M solution is 4.0892 grams.
How to calculate the mass of ammonium sulfide (NH4)2S in the given sample ?
Molarity of the sample = 0.020 M
Volume of ammonium sulfide given = 3.00 L
The number of moles present in a sample is given by -
Number of moles (n) = Molarity (M) * Volume (L)
∴ n = 3 * 0.020 = 0.06.
The number of moles of ammonium sulfide is 0.06.
1 mole of ammonium sulfide (NH4)2S weighs 68.154 g/mole.
∴ 0.06 moles of ammonium sulfide (NH4)2S weighs -
68.154 (g/mole) * 0.06 mole = 4.0892 grams.
Thus the mass of ammonium sulfide (NH4)2S in 3.00 L of a 0.020 M solution is 4.0892 grams.
To learn more about calculating molecular mass of compounds, refer -
https://brainly.com/question/24727597
#SPJ2
