Answer:
3.72 mol Hg
General Formulas and Concepts:
<u>Chemistry - Atomic Structure</u>
- Reading a Periodic Table
- Using Dimensional Analysis
- Density = Mass over Volume
Explanation:
<u>Step 1: Define</u>
D = 13.6 g/mL
54.8 mL Hg
<u>Step 2: Identify Conversions</u>
Molar Mass of Hg - 200.59 g/mol
<u>Step 3: Find</u>
13.6 g/mL = x g / 54.8 mL
x = 745.28 g Hg
<u>Step 4: Convert</u>
<u />
= 3.71544 mol Hg
<u>Step 5: Check</u>
<em>We are given 3 sig figs. Follow sig fig rules and round.</em>
3.71544 mol Hg ≈ 3.72 mol Hg
Answer:
0.46M NaS₂O₃ (Assuming KIO₃ solution with a concentration of 1.0M)
Explanation:
Based on the reaction:
6 Na₂S₂O₃ + KIO₃ + 5 KI + 3 H₂SO₄ → 3 Na₂S₄O₆ + 3 H₂O + 3 K₂SO₄ + 6 NaI
<em>6 moles of Na₂S₂O₃ react per mole of KIO₃</em>
Assuming the molarity of the KIO₃ solution is 0,1M:
Moles of KIO₃: = 5.0x10⁻³L ₓ (0.1 mol / L) = <em>5.0x10⁻⁴ moles</em>
As 6 moles of thiosulfate reacted per mole of iodate:
5.0x10⁻⁴ moles KIO₃ ₓ (6 moles Na₂S₂O₃ / 1 mole KIO₃) =
<em>3.0x10⁻³ moles of Na₂S₂O₃. </em>In 6.5mL (6.5x10⁻³L):
3.0x10⁻³moles Na₂S₂O₃ / 6.5x10⁻³ L = 0.46M NaS₂O₃
Hello!
To know the melting or boiling points of substances is extremely important:
-In a Scientific Setting, it would help identify and separate unknown substances, as the melting or boiling points are unique for each compound, and their determination is useful for identifying and separating them.
-In an Industrial Setting, it would help engineers to know the storage temperatures of compounds. Some compounds if stored at temperatures above their boiling points will evaporate and when stored at temperatures under their melting points will solidify. In some cases this behavior is undesired and knowledge of boiling and melting points is important.
Have a nice day!
First, we distinguish whether table sugar or table salt will be more soluble. The bonds between the molecules of the table sugar are weaker than the bonds between the molecules of salt. Therefore, it is easier for the sugar molecules to dissolve.
Next, we evaluate the effect of temperature on solubility. As the temperature of a solvent increases, it is able to hold more and more solute. This means that the sample with table sugar kept at the highest temperature will contain the most dissolved solute, and this is sample 1.
