Answer:
It would be this below.
Explanation:
I am not 100% sure this is write but I did my best this is still kinda hard for me. I just did this a few years ago and i struggled with it but I have been doing better since then.
Hope this helps :))
To make it easier, assume that we have a total of 100 g of a compound. Hence, we have 58.80g of xenon, 7.166g of oxygen, and 34.04g of fluorine.
Know we will convert each of these masses to moles by using the atomic masses:
58.8/131.3 = 0.45 mole of Xe
7.166/16 = 0.45 mole of O
34.04/19 = 1.79 mole of F
Now, we will divide all the mole numbers by the smallest among them and get the number of atoms in the compound:
Xe = 0.45/0.45 = 1
O = 045/0.45 = 1
F = 1.79/0.45 = 3.98 = 4
So, the empirical formula of the compound XeOF₄
Answer:
Molarity = 12 M
Explanation:
Given data:
Molarity of solution = ?
Number of moles of NaCl = 3.0 mol
Volume of solution = 250 mL (250/1000 = 0.25 L)
Solution:
Molarity is used to describe the concentration of solution. It tells how many moles are dissolve in per litter of solution.
Formula:
Molarity = number of moles of solute / L of solution
Molarity = 3.0 mol / 0.25 L
Molarity = 12 M
Answer: D) 1.00 g
Explanation:
According to the Avogadro's law, the volume of gas is directly proportional to the number of moles of gas at same pressure and temperature. That means,
or,
where,
= initial volume of gas = 2.00 L
= final volume of gas = 3.00 L
= initial moles of gas =
= final moles of gas = ?
Now we put all the given values in this formula, we get
Mass of helium =
Thus mass of helium added = (3.00-2.00) g = 1.00 g
