Answer:
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Explanation:
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I'm pretty sure its metals.
Answer:
The answer to your question is 0.22
Explanation:
Data
Acetonitrile (CH₃CN) density = 0.786 g/ml
Methanol (CH₃OH) density = 0.791 g/ml
Volume of CH₃OH = 22 ml
Volume of CH₃CN = 98.4 ml
Process
1.- Calculate the mass of Acetonitrile and the mass of Methanol
density = mass/ volume
mass = density x volume
Acetonitrile
mass = 0.786 x 98.4
= 77.34 g
Methanol
mass = 0.791 x 22
= 17.40 g
2.- Calculate the moles of the reactants
Acetonitrile molar mass = (12 x 2) + (14 x 1) + (3 x 1)
= 24 + 14 + 3
= 41 g
Methanol molar mass = (12 x 1) + (4 x 1) + (16 x 1)
= 12 + 4 + 16
= 32 g
Moles of Acetonitrile
41 g ----------------- 1 mol
77.34g ------------ x
x = (77.34 x 1) / 41
x = 1.89 moles
Moles of Methanol
32 g -------------- 1 mol
17.40 g --------- x
x = (17.40 x 1)/32
x = 0.54 moles
3.- Calculate the mole fraction of Methanol
Total number of moles = 1.89 + 0.54
= 2.43
Mole fraction = moles of Methanol / total number of moles
Mole fraction = 0.54/ 2.43
Mole fraction = 0.22
The difference between the ideal pressure and the pressure calculated by the Van Der Waal equation is 2.08 atm.
<h3>What is the pressure?</h3>
In this problem, we are mandated to obtain the pressure both by the use of the ideal gas equation and then the use of the Van der Walls equation.
Using the idea gas equation;
PV = nRT
P = nRT/V
P = pressure
V = volume
n = number of moles
T = temperature
R = gas constant
P = 1 * 0.082 * (24 + 273)/0.5
P = 48.7 atm
Using the Van Der Wall equation:
P = RT/(V - b) - a /V^2
P = 0.082 * 297/(0.5 - 0.03219) - 1.345/(0.5)^2
P = 24.354/0.46781 - 1.345/ /0.25
P = 52 - 5.38
P = 46.62 atm
The difference between the ideal pressure and the pressure calculated by the Van Der Waal equation is; 48.7 atm - 46.62 atm = 2.08 atm
Learn more about ideal gas equation:brainly.com/question/3637553
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A goes with u, C with G, and T with A
