Question

In: Chemistry

Assuming that 1.00 L of 4% PVA solution is spread out to form a thin sheet...

Assuming that 1.00 L of 4% PVA solution is spread out to form a thin sheet of thickness equal to the average length of a PVA strand, calculate the total area of the liquid sheet. Then calculate the average of the sheet of solution per strand of PVA. Assuming this area is a little square, the square root of this area gives the edge length of the square which is approximately the average distance between the PVA strands. Show that this distance is about ten times the estimated diameter of a PVA strand (0.2-0.3 nm).

Solutions

Expert Solution

One unit of PVA (monomer) looks like is -(C4H6O2)n-.

The degree of polymerization of polyvinyl acetate (PVA) is typically 100 to 5000.
4% PVA = 40g per litre
Molar mass C4H6O2 = 86g/mol
40g = 40/86 = 0.465 mol
Number of molecules of un-polymerised PVA = 0.465x6.022x1023 = 2.8x1023

If n = 1 in the above formula, then there would be 2.8x1023 particles or strands
If n = 933.3 then there would be (2.8x1023)/933.3 = 3x1020 particles or strands
Where n = the degree of polymerization, which is not given in the question, but it is quite reasonable to have 3x1020 strands of PVA, n = 933 that fits neatly into the range of n = 100 to 5000.

Given the diameter of the PVA strand or particle, d = 0.3x10-9 m

Therefore total length = no. of strands x d = 3x1020x0.3x10-9 = 9x10-10 m

A square has 4 nos. of equal length sides. Therefore the length of the one side (edge length), a = 9x10-10/4 = 2.25x10-10 area

(total area), A = a2

A = (2.25x10-10)2 = 5x10-20 m2

Therefore, area per strand is, a12 = 5x10-20/3x1020 = 1.66x10-40 m2


Related Solutions

Nitrous acid has a Ka of 4.0 * 10-4. in 1.00 L of solution, 0.670 moles...
Nitrous acid has a Ka of 4.0 * 10-4. in 1.00 L of solution, 0.670 moles of nitrous acid (HNO2) are added to 0.281 moles of NaOH. What is the final pH?
Consider a 1.00 L, 1.00 M solution of NaNO3. Will the concentration of NO3- decrease, stay...
Consider a 1.00 L, 1.00 M solution of NaNO3. Will the concentration of NO3- decrease, stay the same, or increase if... A) half of the solution is poured out? B) 500 mL of water is added? C) 500 mL of 1.00M NaNO3 is added? D) 1.00 L of 0.500M NaNO3 is added? E) 1.00 L of 1.00 M NaCl is added? Please show work/explain reasoning
Calculate the pH of 1.00 L of a solution that is 0.120M in HNO2 and 0.150M...
Calculate the pH of 1.00 L of a solution that is 0.120M in HNO2 and 0.150M in NaNO2 before and after you add 2.0mL of 15.0M HCL. [Ka(HNO2) = 4.0 x 10-4]
What is the pH of a 1.00 L buffer solution that is 0.80 mol L-1 NH3...
What is the pH of a 1.00 L buffer solution that is 0.80 mol L-1 NH3 and 1.00 mol L-1 NH4Cl after the addition of 0.070 mol of NaOH(s)? Kb(NH3) = 1.76 ? 10?5
50.0 mL of 2.00 mol/L HNO3 solution and 50.0 mL of 1.00 mol/L NaOH solution, both...
50.0 mL of 2.00 mol/L HNO3 solution and 50.0 mL of 1.00 mol/L NaOH solution, both at 20.0 degree Celsius, were mixed in a calorimeter. Calculate the molar heat of neutralization of HNO3 in kJ/mol if: (1) final temperature was 28.9 degree Celsius; (2) the mass of the overall solution was 102.0 g; (3) the heat capacity of the calorimeter was 25.0 J/C; (4) and assume that the specific heat of solution is the same as water, 4.184 J/(g C);
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.60. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.80. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you 100 mL of 7.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.50. You have in front of you 100 mL of 7.00×10−2M HCl, 100 mL of 5.00×10−2M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution...
Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.50. You have in front of you 100 mL of 6.00×10−2 M HCl, 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT