If you had a pot of boiling water that is loosing volume is that at equilibrium? What are some things you can do to a pot of boi
1 answer:
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Answer:
r= 0.9949 (For 15,000)
r=0.995 (For 19,000)
Explanation:
We know that
Molecular weight of hexamethylene diamine = 116.21 g/mol
Molecular weight of adipic acid = 146.14 g/mol
Molecular weight of water = 18.016 g/mol
As we know that when adipic acid and hexamethylene diamine react then nylon 6, 6 comes out as the final product and release 2 molecule of water.
So
So
Mo= 226.32/2 =113.16 g/mol
Given that
Mn= 15,000 g/mol
So
15,000 = Xn x 113.16
Xn = 132.55
Now by using Carothers equation we know that
By calculating we get
r= 0.9949
For 19,000
19,000 = Xn x 113.16
Xn = 167.99
By calculating in same process given above we get
r=0.995
Answer:
<h2>15 g/mL</h2>Explanation:
The density of a substance can be found by using the formula
But from the question
volume = final volume of water - initial volume of water
volume = 165 - 150 = 15 mL
We have
We have the final answer as
<h3>15 g/mL</h3>Hope this helps you
Answer:
Pressure, P = 67.57 atm
Explanation:
<u>Given the following data;</u>
- Volume = 0.245 L
- Number of moles = 0.467 moles
- Temperature = 159°C
- Ideal gas constant, R = 0.08206 L·atm/mol·K
<u>Conversion:</u>
We would convert the value of the temperature in Celsius to Kelvin.
T = 273 + °C
T = 273 + 159
T = 432 Kelvin
To find the pressure of the gas, we would use the ideal gas law;
PV = nRT
Where;
- P is the pressure.
- V is the volume.
- n is the number of moles of substance.
- R is the ideal gas constant.
- T is the temperature.
Making P the subject of formula, we have;
Substituting into the formula, we have;
<em>Pressure, P = 67.57 atm</em>