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Andrei [34K]
3 years ago
12

An empty 10 ml volumetric flask weighs 10.2634 g. when filled to the mark with distilled water and weighed again in the air at 2

0 oc, the mass is 20.2144 g. what is the true volume of the flask at 20 oc?
Chemistry
2 answers:
Nina [5.8K]3 years ago
7 0
Answer is: <span>the true volume of the flask is 10.2163 grams.
d</span>(H₂O) = 0.9981 g/mL; density of water at 20°C.
V(H₂O) = 10 mL; volume of water.
m(H₂O) = d(H₂O) · V(H₂O).
m(H₂O) = 0.9981 g/mL · 10 mL.
m(H₂O) = 9.9981 g.
m(empty flask) = m(filled flask) - m(H₂O).
m(empty flask) = 20.2144 g - 9.9981 g.
m(empty flask) = 10.2163 g.
Mashcka [7]3 years ago
6 0

Explanation:

It is known that density of water at 20^{o}C is 998,29 kg/m^{3} or 0.998 g/ml (as 1 kg/m^{3} = 0.001 g/ml).

Therefore, calculate mass of water as follows.

        Mass of water = Final mass - initial mass

                                = 20.2144 g - 10.2634 g

                                = 9.951 g

As we known that density is the amount of mass present in a unit volume.                            

Mathematically,       Density = \frac{mass}{volume}

Therefore, putting the given values into the above formula we will calculate the volume as follows.

                         Density = \frac{mass}{volume}

                         0.998 g/ml = \frac{9.951 g}{Volume}

                        Volume = 9.97 ml

Thus, we can conclude that volume of the flask at 20^{o}C is 9.97 ml.

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1) to calculate the limiting reactant you need to pass grams to moles.
<span> moles is calculated by dividing mass by molar mass
</span>
mass of N2O4: 50.0 g 
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</span> 2)</span>
By looking at the balanced equation, you can see that 1 mol of N2O4 needs 2 moles of N2H4 to fully react . So to react  0,54 moles of N2O4, you need 2x0,54 moles of <span>N2H4 moles
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3) 1 mol of N2O4 reacting, will produce 3 mol of N2 (look at the equation)
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4) the only thing left to do is convert the moles obtained, to grams.
We use the same formula as before, moles equal to mass divided by molar mass.
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