It is important to take note of th temperature in determining the density of a substance because this will set as a basis and will likely be a variable in the experiment because this will also contribute on the effects of the experiment and a basis of how the experiment has turned to be that way.
Th actual yield of the reaction is 24.86 g
We'll begin by calculating the theoretical yield of the reaction.
2Na + Cl₂ → 2NaCl
Molar mass of Na = 23 g/mol
Mass of Na from the balanced equation = 2 × 23 = 46 g
Molar mass of NaCl = 23 + 35.5 = 58.5 g/mol
Mass of NaCl from the balanced = 2 × 58.5 = 117 g
From the balanced equation above,
46 g of Na reacted to produce 117 g of NaCl.
Therefore,
11.5 g of Na will react to produce = (11.5 × 117) / 46 = 29.25 g of NaCl.
Thus, the theoretical yield of NaCl is 29.25 g.
Finally, we shall determine the actual yield of NaCl.
- Theoretical yield = 29.25 g
Actual yield = Percent yield × Theoretical yield
Actual yield = 85% × 29.25
Actual yield = 0.85 × 29.25 g
Actual yield = 24.86 g
Learn more about stoichiometry: brainly.com/question/25899385
Most liquids expand when they are heated and contract when they are cooled.
A thermometer consists of a bulb of liquid connected to a thin capillary tube.
When the liquid is heated, it expands and moves up the capillary column. When the liquid cools, it contracts and moves back down the column.
You can determine the temperature by reading the position of the liquid against a graduated temperature scale.
Answer:
Molar mass of the gas = 3.91 g/mol
Explanation:
Let's apply the Ideal Gases Law to solve this:
We convert the pressure from Torr to atm → 885 Torr . 1atm / 760 Torr = 1.16 atm
We convert T°C to T°K → 53°C + 273 = 326 K
We convert the volume from mL to L → 228 mL . 1L/1000mL = 0.228L
Now we can replace = 1.16 atm . 0228L = n . 0.082 .326K
(1.16 atm . 0.228L) / (0.082 / 326K) = n → 9.89×10⁻³ moles.
Let's convert the mass from mg to g → 38.7 mg . 1g / 1000 mg = 0.0387 g
Molar mass → g/mol → 0.0387 g / 9.89×10⁻³ mol = 3.91 g/mol
