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2 years ago

Why was it important not to over-heat the beaker when drying the sodium chloride?

1 answer:

3 0

It important not to over-heat the beaker when drying the sodium chloride so that parts won't be lost, and in addition, if the beaker were to overheat, it would crack.

<h3>Can you evaporate sodium chloride?</h3>

At gas pressures ranging from 0.74 to 212 psia, the rate of evaporation of molten NaCl in the presence of different gases was observed. The rate in crucibles heated by induction had a distinct slope at high and low pressures and was a linear function of (1/P).

It is demonstrated that the (1/P) dependency is predicted for turbulent free convective mass transfer. Under some circumstances, when pressure dropped, the rate of evaporation also did.

This result is explained by the condensation of NaCl in the gas and the subsequent reflux of NaCl particles into the melt. The significant disparity in evaporation rates between Ar, He, and CO2 is related to the CO2's infrared absorption as well as variations in thermal conductivity.

To learn more about properties of sodium chloride from given link

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If element X has 65 protons, how many electrons does it have

Tomtit [17]

In an atom there are the same number of protons as electrons to start with. The answer would be 65 aswell.

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4 years ago

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2 years ago

Calculate the work done when a force of 4 N pulls a box along the floor for a distance of 0.3 m.

Yuki888 [10]

Answer:

<h2>1.2 Joule</h2>

solution,

Force=4 N

Distance=0.3 m

Now,

 $work = f \times d \\ \: \: \: \: \: \: \: \: \: \: \: = 4 \times 0.3 \\ \: \: \: \: \: \: \: \: \: \: \: = 1.2 \: joule$ 

hope this helps...

Good luck on your assignment....

8 0

4 years ago

Which statement is true about the following isotopes: Sulfur-34, Sulfur-33 and Sulfur-32? (Choose all that apply)

Step2247 [10]

Answer:

the different isotopes vary in their relative abundance in nature

8 0

3 years ago

The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolvin

nadya68 [22]

Answer:

(a) 0.039

(b) 0.384 M

Explanation:

We have the following data:

d(C₇H₈) = 0.867 g/mL

d(C₄H₄S) = 1.065 g/mL

V(C₇H₈) = 250.0 mL

mass(C₄H₄S) = 8.10 g

(a) The mole fraction of C₄H₄S in the solution is the number of moles of C₄H₄S divided into the total moles of the solution:

X(C₄H₄S) = moles C₄H₄S/ total moles

To calculate the moles, we need the molecular weight (MW) of each compound:

MW(C₄H₄S) = (4 x 12 g/mol) + (4 x 1 g/mol) + 32 g/mol = 84 g/mol

MW(C₇H₈) = (7 x 12 g/mol) + (8 x 1 g/mol) = 92 g/mol

Thus, we calculate the moles of C₄H₄S by dividing the mass into the MW(C₄H₄S):

moles C₄H₄S = mass(C₄H₄S)/MW(C₄H₄S)= 8.10 g/(84 g/mol) = 0.096 moles

Then, we have to calculate the moles of C₇H₈. First, we need the mass, obtained from the product of the density by the volume:

mass(C₇H₈)= d(C₇H₈) x V(C₇H₈) = 0.867 g/mL x 250.0 mL = 216.75 g

Thus, we divide the mass of C₇H₈ into the MW to calculate the moles of C₇H₈:

moles C₇H₈ = mass(C₇H₈)/MW(C₇H₈) = 216.75 g/(92 g/mol) = 2.35 moles

The total moles is obtained from the addition of the moles of the solute (C₄H₄S) and the solvent (C₇H₈):

total moles = moles C₄H₄S + moles C₇H₈ = 0.096 moles + 2.35 moles = 2.45 moles

Finally, we calculate the mole fraction of C₄H₄S:

X(C₄H₄S) = moles C₄H₄S/ total moles = 0.096 moles/2.45 moles = 0.039

(b) The molarity of C₄H₄S is calculated as follows:

M(C₄H₄S) = moles C₄H₄S/1 liter solution

Assuming that the total volume of the solution is the volume of solvent (C₇H₈), we calculate the molarity of C₄H₄S by dividing the moles into the volume of solvent in liters:

V(C₇H₈) = 250.0 mL = 0.250 L

M(C₄H₄S) = 0.096 moles/(0.250 L) = 0.384 mol/M = 0.384 M

(c) Assuming that the volumes of solute and solvent are additive, we can add the volumes of C₄H₄S and C₇H₈. First, we need the volume of C₄H₄S, which can be calculated from the mass and density:

V(C₄H₄S) = mass(C₄H₄S)/ d(C₄H₄S) = 8.10 g/(1.065 g/mL) = 7.606 mL = 0.0076 L

Now, we add the volumes:

total volume = V(C₇H₈) + V(C₄H₄S) = 0.250 L + 0.0076 L = 0.2576 L

Finally, we recalculate the molarity of C₄H₄S:

M(C₄H₄S)= moles C₄H₄S/ total volume = 0.096 moles/0.2576 L = 0.373 M

7 0

3 years ago