Answer:
the first option: lowering the control rods
Explanation:
i just did it
edge
HAVE A WONDERFUL DAY HONEYS :))
Answer:
0.00552 mol/L
Explanation:
M(FeBr2) = 215.65 g/mol
59.5 mg = 0.0595 g FeBr2
0.0595 g * 1 mol/215.65 g = 0.0002759 mol FeBr2
FeBr2 ------ 2 Br-
1 mol ------ 2 mol
0.0002759 mol FeBr2 * 2 mol Br/1mol FeBr2 = 0.0005518 mol Br-.
100 mL = 0.1 L
0.0005518 mol Br-/ 0.1 L = 0.005518 mol/L≈ 0.00552 mol/L
The magnitude of these forces is directly proportional to boiling and melting points. In addition, molecular polarity<span> affects </span>solubility<span> in that polar molecules are best solvated by polar solvent molecules and nonpolar molecules are best solvated by nonpolar solvent molecules; i.e., "like dissolves like".</span>
The empirical formula is C₇H₆O₂.
Assume that you have 100 g of the compound.
Then you have 68.84 g C and 4.962 g H.
Mass of O = (100 – 68.84 – 4.962) g = 26.20 g O.
Now, we must convert these masses to moles and find their ratios.
From here on, I like to summarize the calculations in a table.
<u>Element</u> <u>Mass/g</u> <u>Moles</u> <u>Ratio</u> <u> ×2</u> <u>Integers</u>
C 68.84 5.732 3.501 7.001 7
H 4.962 4.923 3.006 6.012 6
O 26.20 1.638 1 2 2
The empirical formula is C₇H₆O₂.