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Debora [2.8K]
3 years ago
6

What mass of Neon gas is needed to occupy 2.56 L tube at STP?

Chemistry
1 answer:
malfutka [58]3 years ago
6 0

Answer:

Mass = 2.222 g

Explanation:

Given data:

Volume of  neon gas = 2.56 L

Temperature = 273 K

Pressure = 1 atm

Mass of neon gas = ?

Solution:

PV = nRT

n = PV / RT

n = 1 atm × 2.56 L/ 0.0821 atm. L / mol. K× 273 K

n = 2.56 L.atm / 22.4 atm. L/ mol

n = 0.11 mol

Mass = number of moles × molar mass

Mass = 0.11 mol × 20.2 g/mol

Mass = 2.222 g

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Given what we know, we can confirm that as with any experiment, the control variable will be the one that through each trial of the experiment, no matter how many times it is performed, stays constant.

<h3>What is a controlled variable?</h3>
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If the molar absorptivity constant for the red dye solution is 5.56×104 M-1cm-1, calculate the molarity of the red dye solution
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Explanation:

a) Using Beer-Lambert's law :

Formula used :

A=\epsilon \times c\times l

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c = concentration of solution = ?

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\epsilon = molar absorptivity of this solution =5.56\times 10^4 M^{-1} cm^{-1}

0.945=5.56\times 10^4 M^{-1} cm^{-1}\times 1.20 \times c

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14.16 μM is the molarity of the red dye solution at the optimal wavelength 519nm and absorbance value 0.945.

b) c=1.4163\times 10^{-5} mol/L

1 L of solution contains 1.4163\times 10^{-5} moles of red dye.

Mass of 1.4163\times 10^{-5} moles of red dye:

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c) In order to dilute red dye solution by 5 times, we will need to add 1 L of water to solution of given concentration.

Concentration of red dye solution = c=1.4163\times 10^{-5} M

Concentration of red solution after dilution = c'

c=c'\times 5

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c'=2.83\times 10^{-6} M

The final concentration of the diluted solution is 2.83\times 10^{-6} M

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